Unit 2:1 Properties of Matter - · PDF fileUnit 2:1 Properties of Matter Density 30 g 10 g If...

Name: _____________________

Period: _____________________

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Unit 2:1

Properties of Matter

Density

30 g 10 g

If two objects have the same

size (volume) the one with

more mass is denser.

This one

is denser.

30 g 30 g

If two objects have the same

mass the smaller one

(less volume) is denser.

This one

is denser.

Density is how compact an object is. Density is a measure of how tightly packed the

atoms of a substance are. More tightly packed atoms make a denser substance.

A ping-pong ball and a golf

ball are approximately the

same size, but the golf ball

is heavier, so it is denser.

D = m

v

is a formula. Put the number in the cor-

rect part of the formula to find density.

Density: in g/mL or

g/cm3

Mass in grams (g)

Volume in

cm3 or mL

Density = Mass ÷ Volume

D = m

v Ex. An 20 gram object has a volume of 5 cm3.

Find its density.

Solution:

3 3

204

5

m g gD

V cm cm= = =

Hardness Brittleness How difficult it is to

scratch something.

A diamond is very hard

because you can’t scratch it.

Soap is easy to

scratch, so it is not hard.

How easy it is to shatter

when dropped or struck.

Wood is not very brittle

because it will not shatter if dropped.

Elasticity How much something can bend

and return to its original shape.

How easy it is to pound

something into thin sheets.

Glass is brittle because it

will easily shatter if dropped.

Rubber is very elastic because

it can stretch without breaking. Gold is very malleable because you

can pound it into very thin sheets.

Malleability

Ice is not malleable because

it will shatter instead of spread out.

A pencil is not elastic because

it will break if you bend it.

Viscosity How slowly a liquid pours. Tensile Strength How hard it is to break

something by pulling it.

Syrup pours very slowly,

so it is very viscous.

Water pours quickly,

so it is not viscous.

Spider webs can be pulled very hard before

they break. Spider webs have more tensile

strength than steel cables.

Tissue paper is easily pulled apart,

so it has very little tensile strength..

Name: _____________________

Period: _____________________


Unit 2:1

Substance Dense? Brittle? Viscous? Malleable? Elastic? Hard? Tensile

Strength?

Glass medium yes N/A no no yes high

Rubber

Ice

Molasses

Steel

Styrofoam

In science we describe substances and their various properties. Each substance has many different properties.

Fill in the following table, deciding how each property best describes the following substances.

1. Density

2. Hardness

3. Brittleness

4. Elasticity

5. Malleability

a. A measurement of how easily a solid can be pounded into thin sheets

b. A measurement of the “compactness” of a substance; ratio of mass to volume.

c. Measure of a solid’s ability to return to its original shape after stretching.

d. A measure of how easily a solid will shatter.

e. A measure of how easily a solid can be scratched.

1.Tensile

Strength

2. viscosity

3. cm3

4. g/mL

5. ÷

A. A unit of volume that equals 1 mL.

B. In a formula, what the horizontal line means: ex. the line in:

C. Measure of a fluid’s resistance to flow. (How thick a fluid is.)

D. Measure of how hard it is to break something by pulling.

E. Unit of density.

A soccer ball and a

bowling ball are

approximately the

same size.

Which one is denser?

Why?

When building a bridge, engineers want the bridge cables

to have great _________________.

Glass can be scratched by quartz. Which one is harder?

Lead feels very heavy for its size. It is very __________.

Transmission fluid is a very thick oil that flows slowly.

Transmission fluid is very _____________.

When a fluid gets hotter, do you think it will be more or

less viscous? (Think of warmed-up syrup.)

When gold is hammered it “squishes”. Iron Pyrite is

known as “Fool’s Gold”. It is not ___________ like gold,

but shatter into many pieces when struck by a

hammer. Iron Pyrite is __________.

A hunter’s wood bow stores energy that is given to the

arrow. The wood’s ability to springs back means it is

very ___________.

An object has a volume of 3.5 cm3 and a mass of

7 grams. Find the object’s density.

If 60 grams of a liquid takes up 120 mL, how dense

is the liquid?

Object A Object B Which object is the

most dense?

Why?

Challenge: If a substance has a density of 2.5 g/cm3,

how much mass will 50 cm3 of it have?

m

v

50 g 50 g

Name: _____________________

Period: _____________________


Name: _____________________

Period: _____________________


Unit 2:2

Measuring Density

Density: in g/mL or

g/cm3

Mass in grams (g)

Volume in

cm3 or mL

Density = Mass ÷ Volume

D = m

v

The density of an object

is defined as how

compact it is. To find

an object’s density, you

must measure its mass

and volume. Measuring the mass of a solid

is simple with a balance scale.

Displacement Method The displacement method allows you to easily and quickly measure the mass

of an object by measuring how much water it displaces.

Mass of a Liquid You can’t measure a liquid by putting it on a scale.

You must measure it while it is inside a container.

Mass with liquid − Mass empty = Mass of liquid

450g − 300 g = 150 g

The liquid has a mass of 150 g.

Before (empty)

mempty = 300 g After (with liquid)

mwith fluid = 450 g

The beaker has more mass afterwards,

since it has a liquid in it.

Before

(Just water)

Vbefore = 16 mL

After

(With object)

Vafter = 26 mL

Volume after − Volume before = Volume of object

26 mL − 16 mL = 10 mL

The object has a volume of 10 mL.

The water went up because

the object displaced the water.

Floating Objects If an object floats, it is necessary to submerge it, push it into the water in order to

use the displacement method to find its volume.

The object

floats, so you

can’t find its

volume easily.

Push the object into

the water until the

top of it is at the top

of the water

Use the displacement method when an object is hard to

measure because it has a strange or irregular shape.

OR use the displacement method for regular objects just

because it is easy and fast.

10

30

20

10

30

20

Sinking an object—

If an object is hollow and has

a water tight lid you could fill

it with a denser object and

sink it. Be sure to take the

mass of the empty container to

find its density, though.

Name: _____________________

Period: _____________________


Unit 2:2

How do you measure the mass of a solid?

How do you measure the mass of a liquid?

How do you measure an irregular shaped object?

How do you measure the volume of a floating object?

5

15

10

5

15

10

5

15

10

5

15

10

Volume before: ________ Volume after: ________

Volume of the toy car: ______________

If the mass of the toy car is 14 grams, find its density.

Empty mass: 65 grams Mass with liquid: 88 grams

Volume of liquid: _______

Mass of the just the liquid: ___________________________

What is the density of the liquid?

5

15

10

5

15

10

Empty mass:

20 grams

With water:

31 grams

Find the density

of the liquid in

the cylinder.

Empty mass:

65 grams

With Liquid A:

73 grams

5

15

10

5

15

10

5

15

10

With liquid B:

71 grams

The two liquids have the same: ______________

Which one has more mass? _________________

Volume of A: ______ Mass of A: ___________

Density of Liquid A: ______________________

Volume of B: ______ Mass of B: ___________

Density of Liquid B: ______________________

5

15

10

What is the

volume of

the object?

5

15

10

Name: _____________________

Period: _____________________


Name: _____________________

Period: _____________________


Unit 2:3

More Density

Less Dense Objects Float

Heavy things don’t sink

(unless they are denser).

A ship is heavy, but it floats in

water because it is less dense.

Light things don’t float

(unless they are less dense).

A penny is light, but it sinks in

water because it is more dense.

If two objects are put together, the less dense one will float.

You can tell by the numbers, too. If the object’s density < Liquid’s density, the object will float.

Ex. 1 Object A: D = 1.56 g/mL

Liquid B: D = 1.2 g/mL

The object sinks! (It is more dense.)

Ex. 2 Object A: D = 0.85 g/mL

Liquid B: D = 1.0 g/mL

The object floats! (It is less dense.)

States of Matter and Density For the same substance the three states of matter

have different energies and different densities.

Liquids: Medium energy; medium

density. Molecules slide around,

staying close together.

Solids: Low energy; high density.

Molecules are stuck together.

Gases: high energy; low density.

Molecules bounce around,

spreading out.

Density of Water = 1 g/mL

This means that every mL of water = 1 g

OR every gram of water = 1 mL

This makes calculations

with water easy.

Vwater (in mL) = mwater (in g)

Ex. 35 g water = 35 mL

46 mL of water = 46 g

Density of Ice = 0.92 g/mL

Ice is less dense than water.

Water is the ONLY substance

whose solid floats in its liquid.

Water

D = 1 g/mL

Ice

D = 0.92 g/mL

Water: The Exception Solid water floats

in liquid water.

Floating Ice is Important for Life

Floating ice on lakes and ponds

insulates fish during cold winters.

The expansion of water freezing

breaks down rocks into soil.

G a s e s

Liquids

Solids

Mo

re E

ner

gy

Mo

re Den

se

Solid wax

Solids sink in their liquids.

Solids are denser than their liquids.

Liquid wax

Density Columns

Least Dense

Most Dense

Liquid B is more dense than Liquid A.

Liquid C is more dense than Liquid B.

A

B

C

By putting an object into the

column you can estimate its density

by where it floats or sinks.

This object has a density

greater than liquid B, but

less than liquid C.

When different liquids are put

together in a column they

separate due to their different

densities. If they are put in a

different order, they will still

end up in the right order.

Name: _____________________

Period: _____________________


Unit 2:3

1. Solids

2. 1.0 g/mL

3. Gases

4. 0.92 g/mL

5. Density Column

6. Liquids

7. Ice

A. Only solid that floats in its liquid.

B. Tightly packed atoms; very dense.

C. Loose atoms; low density.

D. Density of water.

E. Separates liquids by density.

F. Density of ice.

G. Close atoms; medium density.

Sinks or Floats in Water?

True or False? If false, correct the statement.

Light things float.

Heavy things sink.

Liquid wax or solid wax?

Solid water or liquid water?

Liquid iron or solid iron?

Liquid nitrogen or gaseous nitrogen?

Circle the one that is more dense.

__ D = 1.2 g/mL

__ Ice

__ D = 0.85 g/mL

__ Styrofoam

__ A rock

__ D = 2.2 g/mL

C

B

A

Which liquid is the most dense? A, B, or C?

Which liquid is the least dense? A, B, or C?

Which liquid is which? A, B, or C?

D = 1.35 g/mL = Liquid ___

D = 0.86 g/mL = Liquid ___

D = 1.00 g/mL = Liquid ___

Label the liquid you know.

Draw where ice will float in the column.

Fill in the following table for the liquids you are given.

Your Final Density Column

What is the density of water?

If you have 30 grams of water, how

many mL of water do you have?

How many grams is 23 mL of water?

How many grams of water is in the

graduated cylinder?

Liquid Mass Volume Density

In what order do you think the liquids will stack?

Mass of empty cylinder:

List the solid objects

you have been given

from least dense to

most dense (guessing).

In the Lab

Empty: 12 grams

10

15

5

With Liquid A: 24 grams

10

15

5

With Liquid B: 28 grams

10

15

5

Mass of Liquid A: ________________

Volume of Liquid A: ______________

Density of Liquid A: ______________

Mass of Liquid B: ________________

Volume of Liquid B: ______________

Density of Liquid B: ______________

Which one would float on top?

Name: _____________________

Period: _____________________


Name: _____________________

Period: _____________________


Unit 2:4

Buoyancy and Archimedes’ Principle

A warning buoy is

buoyant (it floats).

1. A 60 g object seems to be only 40 g when

put into a liquid. How much buoyancy did

the liquid give?

2. A 150 g object seems to be only 110 g when

put into a liquid. How much buoyancy did

the liquid give?

3. If an object displaces 20 mL of water.

What is the mass of the displaced water?

4. If an object has 76 grams of mass,

how much water must it displace to float?

5. A 125 gram object displaces 100 grams of water.

Will it sink or float?





One step farther...

8. A 60 gram ship displaces 90 grams of water.

How much cargo can it hold before it sinks?





Buoyancy—the upward force of a fluid on an object.

When an object is put into a fluid, it feels lighter

because the fluid pushes up on the object. This is

known as the buoyant force.

A denser liquid (usually more viscous) will give more

buoyant force.

A more buoyant object floats better.

A less dense object is more buoyant.

100 g 60 g

The mass seems lighter in the liquid.

The liquid pushes up on the mass,

giving buoyant force.

Buoyant force = weight not in fluid – weight in fluid

Ex. A 35 Newton object seems to weigh 30 Newtons in water.

35 N – 30 N = 5 Newtons (the buoyant force given by the water)

Archimedes Principle

Ex 1. A 50 gram object displaces

50 grams of water (50 mL).

It will float.

Ex 2. A 65 gram object displaces

64 grams of water (64 mL).

It will sink.

Remember:

Noah’s Ark floated

because of

Archimedes’ Principle.

Steel ship;

Air

Same mass

More volume

Less dense, so

it will float!

Same mass Less volume

higher density. It will sink.

Steel block

In order for something to float it must

displace enough fluid to equal its weight.

A ship floats because of its shape. With

air in the middle of the ship it displaces

(pushes away) enough water to equal

its mass. A 12 ton ship must displace

at least 12 tons of water to float.

Name: _____________________

Period: _____________________


Unit 2:4

Buoyancy Lab—Archimedes’ Principle

1) Find the initial mass of the balloon system (balloon with 20 pennies and the binder clip). Record in data table below.

2) How much water will have to be displaced for the balloon system to float? Record below.

3) Level the overflow tank this way:

From the large beaker pour water into the displacement tank until it pours out into the small beaker.

When the water stops flowing into the small beaker, empty the small beaker into the large beaker.

4) Seal the uninflated balloon system with the clip. Put it into the displacement tank and let the water flow into the small beaker.

5) With the graduated cylinder, determine how much water mass the balloon system displaced. Record below.

6) Did the balloon system float or sink? Record below.

7) Retrieve the balloon system. Relevel the overflow tank as in procedure 3).

8) Inflate the balloon just smaller than a tennis ball; seal with the clip; find the water mass displaced. Record below.

9) Relevel the overflow tank as in procedure 3).

10) Inflate the balloon to the size of a baseball (but smaller than the displacement tank). Record the water mass displaced:

QUESTION: Archimedes’ Principle states that the balloon will float if the water it displaces equals the mass of the object.

Did this happen? Record below.

11) Find the volume of the film canister. Record below.

12) Using Archimedes’ Principle determine what the maximum mass the canister can hold and still float. Record below.

13) Measure the mass of one penny: Record below.

14) Predict how many pennies will float in the canister? Record below.

15) Test your hypothesis. Record your data below.

1) Mass of balloons and pennies

2) Volume of water needed to hold up balloon and pennies

5) First amount of water displaced

6) Float or sink?

8) Second amount of water displaced

10) Third amount of water displaced

Q: Archimedes' Principle

11) Film canister volume

12) Maximum mass before the canister sinks.

13) Mass of one penny

14) Prediction of how many pennies will float.

15) Maximum # of pennies before it sank.

DATA TABLE

Name: _____________________

Period: _____________________


Name: _____________________

Period: _____________________


Unit 2:5

Atoms, Elements, Molecules, and Compounds

Our modern model of the atom comes from the contributions of several scientist over millennia.

5. In 1913 Niels Bohr, while studying light, realized that electrons can only exist in certain energy levels or orbitals.

Atoms, Elements, Molecules, and Compounds

Compounds

A compound is any

combination of two or more

different atoms. All

compounds are molecules.

3 atoms

2 elements

1 molecule

1 compound

A molecule is any

combination of two or

more atoms. Not all

molecules are compound.

2 atoms

1 element

1 molecule

0 compounds

An element has only

one kind of atom. All

elements are found on the

periodic table of elements.

4 atoms

3 elements

1 molecule

1 compound

Elements

H

O

H

O O C

O He

He

Atoms

An atom is a single

piece of an element

that retains the

element’s properties.

Cl

Mg

Cl

3 atoms

2 elements

1 molecule

1 compound

4. The nucleus was discovered in 1911 when Ernest Rutherford shot alpha particles at gold foil. Most of the particles passed thru the foil, since the atom is mostly empty space with a solid, central nucleus.

The Atom

1. The Greek scientist Democritus (BC 460-370) proposed that there had to be a smallest part of matter, which he called atomos (indivisible).

2. In 1808 John Dalton published a theory of the atom that had these important points:

• All atoms of a particular element are the same.

• Atoms of different elements have different properties, mass, and chemical reactivity.

• Atoms are not changed by chemical reactions, just rearranged in order or number.

3. Electrons were discovered by J.J. Thomson in 1897. By watching streams of particles bend toward positive plates, he realized the particles were negative. Knowing atoms were neutral, he thought that electrons were like negative plums in positive pudding.

–

+

+ +

+ –

– –

Thomson: plum pudding atom: negative plums (electrons) in the positive pudding (atom).

Democritus: Indivisible atoms are hard spheres.

Dalton: Each element’s atoms are the same.

Rutherford: the atom is mostly empty space with a solid nucleus.

negative electrons Central

nucleus

nucleus: contains positive protons

and neutral neutrons

negative electrons

electron orbitals (energy levels).

Electrons cannot exist between

levels.

Niels Bohr model of the atom.

6. Scientists have now split the atom and even split protons, neutrons, and electrons into even smaller particles called quarks.

Particle Charge Location Mass Tells the

proton positive Nucleus 1 amu element

neutron neutral Nucleus 1 amu isotope

electron negative Orbitals 1/2000 amu ion

Subatomic Particles

Subatomic means

“smaller than the atom”.

Each particle has different

properties and locations.

Molecules

Name: _____________________

Period: _____________________


Unit 2:5

1. Proton.

2. Neutron

3. Electron

4. Nucleus

5. Atom

A. Particles with no charge found in the nucleus of atoms.

B. Center of the atom; contains protons and neutrons.

C. Positively charged particle in the nucleus of the atom. Determines the element.

D. The smallest part of an element or molecule. Building block of all things.

E. Negative particles in orbits around the atom.

1. Molecule

2. Compound

3. Atom

4. Element

A. Smallest part of an element. Can only be split by nuclear means.

B. Any combination of two or more elements.

C. Any combination of two or more atoms, whether the same or different.

D. A substance in which all the atoms are the same.

1. Dalton

2. Bohr

3. Democritus

4. Rutherford

5. Thompson

A. Discovered that atoms have a nucleus.

B. Discovered the electron.

C. Realized that there was a smallest part of matter.

D. Discovered that electrons are in distinct orbits.

E. Theorized that atoms cannot be changed chemically.

Draw a picture of an atom, using the Bohr model. Be sure to

label the nucleus, protons, neutrons, electrons, and orbitals.

O

C

O

F F

Li

Li Li

N

S

O O O

H K

Atoms: ___

Elements: ___

Molecules: ___

Compounds: ___

Atoms: ____

Elements: ____

Molecules: ____

Compounds: ___

Atoms: ____

Elements: ____

Molecules: ____

Compounds: ___

Atoms: ____

Elements: ____

Molecules: ____

Compounds: ____

Atoms: ____

Elements: ____

Molecules: ____

Compounds: ____

1 electron (e): _________

1 proton (p): __________

1 neutron (n): _________

2 electrons (2 e) : ______

4 protons (4 p): ________

3 neutrons (3 n): _______

2 p + 2 e: _____________

4 p + 2 n: ____________

1 n + 3 p: ____________

3 p + 3 n + 2 e: ________

6 p + 7 n + 8 e: ________

9 p + 10 n + 10 e: ______

Give the charges for the following:

Name the subatomic particles that make up the atom.

The number of protons tells you the ________________ .

The number of electrons tells you the _______________ .

The number of neutrons tells you the _______________ .

How did the Rutherford experiment prove the existence of

the nucleus?

Ca

20

40.078

Atomic #

(number of

protons)

Find the atomic number of:

A) Fe: _______

B) K: _______

C) Ni: _______

D) Al: _______

Find the elements:

A) 8 protons: ________

B) 6 protons: ________

C) 15 protons: ________

D)86 protons: ________

Name: _____________________

Period: _____________________


Name: _____________________

Period: _____________________


Unit 2:6

Isotopes and Making Atoms

Electrons Orbits Electrons will want fill up inner orbits first to get as close to the nucleus as possible.

They also want to stay as far away from each other as possible.

3p 3n

lithium

Correct! - Inner orbit

is full (with 2);

one outer electron.

lithium

3p 3n

Incorrect! - The electrons will

fill up the inner levels first.

The first level takes 2 electrons.

– +

proton electron

Opposites

attract – –

Like charges

repel

2 electrons

Ions and Neutral Atoms

Ions

If the number of electrons equals the number of

protons the atom is neutral. If not, it is an ion.

Neutral Atoms

2 protons = Helium 2 proton (+2)

2 electrons (–2) +2 –2 = 0

neutral atom

1 proton = Hydrogen 1 proton (+1)

1 electrons (–1) +1 –1 = 0

neutral atom

11 protons = Sodium

11 p –10e = +1

positive ion: Na+1

11p 12n

8p 8n

8 protons = Oxygen

8 p –10e = –2

negative ion: O –2

Positive and

negative

ions attract

each other.

attract

2nd level

3rd level

1st level

4th level

# rows = # of energy levels.

End of a row means a full energy level.

Neon has 2 filled energy levels.

The # of elements in a row = # of

electrons in a level.

Sodium starts the 3rd electron levels.

1st row has 2 elements, so the first energy level can hold 2 electrons.

Isotopes of Hydrogen

Because they each have

1 proton, they are all

hydrogen atoms, but are

different isotopes

because they have

numbers of neutrons .

Protons

Hydrogen 1

1p + 0n = 1

Hydrogen 2

1p + 1n = 2

Hydrogen 3

1p + 2n = 3

Neutrons Isotopes of Beryllium

Isotopes An isotope is a variation of an element. It has the same number of protons

(same element), but a different number of neutrons (different isotope).

4p 4n

4p 5n

Beryllium 8

4p + 4n = 8

Beryllium 9

4p + 5n = 9

Atomic number

(number of protons)

Finding the # of Neutrons

Mass # = protons + neutrons

Neutrons = mass # – protons

For Hydrogen 3:

3 (mass #) – 1 (atomic #) = 2 (neutrons)

Hydrogen 3 has 2 neutrons.

Atomic mass (average of all the isotopes)

Mass numbers (Most common isotopes)

Reading the Tiles

The atomic mass

is an average.

Round it to

find the most

common isotope.

Hydrogen

1

H 1.01 1, 2, 3

Name: _____________________

Period: _____________________


Unit 2:6

1. Isotope

2. Atomic mass

3. Atomic #

4. Neutral atom

5. Ion

6. Mass #

A. An average of all the isotopes; the mass of average atom.

B. An atom with an equal number of electrons and protons.

C. An atom with more or less electrons than protons.

D. A variation of an element with a different number of neutrons.

E. Total number of protons and neutrons in the nucleus.

F. Number of protons; determines the element.

7 protons and 10 electrons. Neutral atom or ion?




Give the element abbreviation and charge.

5 protons and 2 electrons: Element: B Charge: +3 .

16 protons and 18 electrons: Element: Charge: .



Calcium (Ca) 20 .

Potassium (____)________

Copper (____) __________

Zirconium (____) _______

Boron (____) __________

Selenium (____) _______

Silver (____)___________

Mercury (____) ________

Give abbreviations and number of protons

Which of the following are isotopes?

Element A: 15 protons; 15 electrons; 16 neutrons

Element B: 14 protons; 16 electrons; 14 neutrons

Element C: 15 protons; 18 electrons; 15 neutrons

Element D: 16 protons; 18 electrons; 15 neutrons

Element E: 15 protons; 18 electrons; 14 neutrons

Sulfur 32 has 16 protons and 16 neutrons. (32 – 16p = 16n)

Magnesium 25 has ___ protons and _________ neutrons.

Carbon 14 has ___ protons and _________ neutrons.

Lithium 7 has ___ protons and _________ neutrons.

Chlorine 35 has ___ protons and _________ neutrons.

Fluorine 19 has ___ protons and _________ neutrons.

Oxygen 16 has how many neutrons?

Beryllium 8 has how many neutrons?

Boron 11 has how many neutrons?

10p 11n

This picture is supposed to

be of a neutral atom. Fix it.

neutron

proton

electron

What’s wrong with this

picture of an atom?

8p 7n

What is wrong with this

picture of an atom?

7p 7n


picture of an atom?

Which row is Lithium (Li) in? 2 . It has electrons in levels

1 and 2.

Which row is phosphorous (___) in? ____ So, phosphorous

has electrons in which electron levels?

Which row is calcium (___) in? ____ So, calcium has

electrons in what levels?

Which row is argon (___) in? ____ So, argon has electrons

in what levels?

Argon (___) is at the end of row ___. So argon has ____

full electron levels.

Helium (___) is at the end of row ___. So helium has ____


Xenon (___) is at the end of row ___. So xenon has ____


How many full electron levels does Calcium have?

How many full electron levels does Sulfur have?

Name: _____________________

Period: _____________________


Name: _____________________

Period: _____________________


Unit 2:7

Metals, Non-Metals and Valence Electrons

1

H

3

Li

19

K

11

Na

4

Be

20

Ca

12

Mg

1A 18A

2A 13A 14A 15A 16A 17A

1

2

3

4

Electron

Levels

(Periods)

5

B

31

Ga

13

Al

6

C

32

Ge

14

Si

7

N

33

As

15

P

8

O

34

Se

16

S

9

F

35

Br

17

Cl

2

He

10

Ne

36

Kr

18

Ar

Groups

Transition Metals (valence electrons vary)

Groups

1

2

8

3 5 4 6 7

3 5 4 6 7 8 1 2

Valence Electrons

Divides

metals and

non-metals

Metals Non-metals

Valence Electrons Valence Electrons are the outermost electrons in an atom.

Each group (column) has the same number of valence electrons.

Only valence electrons are involved in chemical bonding.

1p

Hydrogen 1

1 valence electron

3p 3n

Lithium 6

1 valence electron

Hydrogen and Lithium are both in

Group 1A—both have 1 valence electrons.

Octet Rule – Atom are

more stable that have a full

shell of electrons. For most

atoms 8 valence electrons is

full (octed = 8). For H and

He this number is 2. Atoms

want to have 8 valence

electrons. “If I 8, I full.”

Only elements in Group

18A have a full octet

(8 valence electrons)

naturally. All other

elements will lose, gain,

or share to reach 8 electrons.

Oxygen 17

8p 9n

6 valence electrons

Inner electrons

are NOT

valence electrons

Metals and Nonmetals

Metals are on the left side of the periodic

table. Non-metals are on the right side.

Metals and non-metals have different

properties and bond differently,

making different kinds of compounds.

Metals or Non-metal?

Calcium (Ca): metal (left side)

Bromine (Br): non-metal (right side)

Along the separation line are

the semimetals or metalloids:

Boron (B), Silicon (Si),

Germanium (Ge), Arsenic

(As), Antimony (Sb). These

have properties of both

metals and non-metals.

Going Farther

Elements with the same valence electrons have

similar reactivity, so they tend to react the same.

Exception:

Helium

only has 2

valence

electrons!

Name: _____________________

Period: _____________________


Unit 2:7

1. Octet Rule

2. Metals

3. Valence

electrons

4. Non-metals

A. Elements found on the right side of the periodic table.

B. Elements found on the left side of the periodic table.

C. Says that atoms tend to be more stable with eight valence electrons.

D. Electrons in the outermost electron level. Involved in chemical bonding.

Calcium (Ca) 2 .

Potassium (____)________

Oxygen (____) _________

Argon (____) __________

Boron (____) ___________

Hydrogen (____) _______

Helium (____) _________

Aluminum(____) _______

Sodium (____) _________

Nitrogen (____) ________

How many valence electrons?





5 protons and 2 electrons: Element: B Charge: +3 .



Metal or Non-metal?

__M__ Aluminum ( Al )

____ Oxygen (___)

____ Gold (___)

____ Nitrogen (___)

____ Bromine (___)

____ Krypton (___)

____ Iron (___)

____ Fluorine (___)

____ Tin (___)

____ Lithium (___)

____ Chromium (___)

____ Lead (___)

Connect the element on the left with the element

on the right that has similar reactivity.

Are these elements isotopes of one another?

Element A: 12 protons; 11 electrons; 13 neutrons.

Element B: 13 protons; 12 electrons; 13 neutrons.










10p 11n

11p 12n

Element: _______________

# of neutrons: ___________

Mass #: ________________

# of electrons: ___________

# of valence electrons: ____

It is an ion? _____________

2p 2n

Element: _______________

# of neutrons: ___________

Mass #: ________________



It is an ion? _____________

Element: _______________

# of neutrons: ___________

Mass #: ________________



It is an ion? _____________

Sulfur (_S_) is in row __3__. Sulfur has __2___ complete

electron levels and __6_ valence electrons in level __3___.

Magnesium (____) is in row ____. Magnesium has _____

complete electron levels and _____ valence electrons in

level _____.

Carbon (____) is in row ____. Carbon has _____ complete

electron levels and _____ valence electrons in level _____.

Potassium (___) is in row ____. Potassium has ____

complete electron levels and _____ valence electrons in

level _____.

Argon (____) is in row ____. Argon has _____ complete


Chlorine

Phosphorous

Magnesium

Sodium

Boron

Sulfur

Beryllium

Potassium

Iodine

Aluminum

Oxygen

Nitrogen

Elements with the

same # of

__________

__________ have

the same reactivity.

Name: _____________________

Period: _____________________


Name: _____________________

Period: _____________________


Unit 2:8

Properties of Matter Review

1. Density

2. Brittleness

3. Hardness

4. Elasticity

5. Malleability

a. A measure of how easily a solid can be scratched.

b. A measurement of how easily a solid can be pounded into thin sheets.

c. A measurement of the “compactness” of a substance; ratio of mass to volume.

d. Measure of a solid’s ability to return to its original shape after stretching.

e. A measure of how easily a solid will shatter.

1.Tensile

Strength

2. viscosity

3. cm3

4. 5. ÷

5. g/mL

A. A unit of volume that equals 1 mL.

B. Measure of a fluid’s resistance to flow. (How thick a fluid is.)

C. Measure of how hard it is to break something by pulling.

D. Unit of density.

E. In a formula, what the horizontal line means: ex. the line in:

Object A Object B Which object is the

less dense?

Why? 50 g 50 g

Which object is the

less dense?

Why? 50 g 80 g

Object A Object B

A 15 g object has a volume of 30 cm3. Find its density.

A 12 g object has a volume of 6 mL. Find its density.

A 35 mL object has a density of 2 g/mL. Find its mass.

A rock climber wants a rope with great ________________.

An airplane pilot wants a windshield that is ___________.

A child bends a toy. It stays bent because it wasn’t very

__________.

I step on a ball of aluminum foil. The aluminum flattens

because it is very ______________.

In Alaska, cars need oil that is thinner and flows faster, so

during the cold winter it doesn’t become too ___________.

Balsa wood is very light for its size, so it is not very _______.

We give small children plastic dishes because ceramic dishes

are too _________ and break too easily

A piece of wood floats because it has ______________.

How do you measure the mass of a liquid?

How do you measure the volume of a floating object?

What is the volume of the object?

What is the object’s density?

5

15

10

5

15

10 12 grams

C

B

A

Which liquid is which? A, B, or C?

D = 1.00 g/mL = Liquid ___

D = 0.75 g/mL = Liquid ___

D = 1.83 g/mL = Liquid ___

Label the liquid you know.

Draw where ice will be in the column.

In the column, where would a cube of

density 0.89 be?

Which is more dense: liquid iron or solid iron?

Which is more dense: gaseous CO2 or liquid CO2?

Which is more dense: liquid water or solid water?

A 200 g object displaces 150 g of water. Float or sink?

A 300 g object displaces 350 g of water. Float or sink?

A 250 g object displaces 300 g of water. How much cargo

can it hold?

Name: _____________________

Period: _____________________


Unit 2:8

Helium (____) _________

Calcium (____) _________

Sulfur (____) __________

Lithium (____) _________

Aluminum (____) _______

Nitrogen (____) _________

How many valence electrons?



20 protons and electrons. Neutral atom or ion?




Nitrogen with 10 electrons. Charge: _________.

Metal or Non-metal?

____ Titanium (___)

____ Sodium (___)

____ Chlorine (___)

____ Neon (___)

____ Hydrogen (___)

____ Nickel (___)

Are these different elements?



Why?

Are these different isotopes of one another?



Why?

Are these different isotopes of one another?



Why?

12p 13n

Element: _______________

# of neutrons: ___________

Mass #: ________________


# of valence electrons: _____

It is an ion? _____________

Calcium (___) is in row ____. Calcium has _____ complete


Sulfur (____) is in row ____. Argon has _____ complete


A 35 N object feels like 30 N when lowered into a liquid.

How much b______ force does the liquid give?

If put into a more v_______ liquid, the object would feel

even lighter.

Calcium and ___________ have the same reactivity.

Oxygen and ___________ have the same reactivity.

Helium and ___________ have the same reactivity.

1. Bohr

2. Dalton

3. Democritus

4. Rutherford

5. Thompson

A. Discovered that atoms have a nucleus.

B. Realized that there was a smallest part of matter.

C. Discovered that electrons are in distinct orbits.

D. Discovered the electron.

E. Theorized that atoms cannot be changed chemically.

1. Isotope

2. Atomic mass

3. Atomic #

4. Neutral atom

5. Ion

6. Mass #

A. An average of all the isotopes; the mass of average atom.

B. An atom with an equal number of electrons and protons.

C. An atom with more or less electrons than protons.

D. A variation of an element with a different number of neutrons.

E. Total number of protons and neutrons in the nucleus.

F. Number of protons; determines the element.

Be

For all of the above:

Atoms: _______

Elements: _______

Molecules: _______

Compounds: _______

8p 7n


picture of an atom?

“Atoms are solid.” Respond and give reasons for your

response.

Name: _____________________

Period: _____________________


Name: _____________________

Period: _____________________


Electrons are not as close

to protons as possible

(should fill in inner

levels first

Name: _____________________

Period: _____________________


In this Investigation you will:

- Find the density of various liquids.

- Approximate viscosity of various liquids.

- Make a density column of liquids.

- Use the density column to approximate the density of solids.

Lab Safety:

Goggles: to protect your eyes from the various liquids.

Apron: to protect your clothes.

Pre-Lab Review (Answer these 5 questions first):

What two measurements do we need to find density?

What is the equation for density?

If the density of a solid is less than the density of a liquid will it:

sink or float? (pick one)

If the density of a solid is more than the density of a liquid will it:

sink or float? (pick one)

A liquid of greater viscosity will flow slower or faster?

Procedure 1: Measuring the Density of the Five Liquids

Find the mass of the 10 mL plastic graduated cylinder and record in the table.

Using the plastic cylinder find the mass and volume of each of the five liquids and

record in the table.

Remember to rinse the graduated cylinder between each liquid.

Calculate the density of each liquid.

Procedure 2: Predicting How to Stack the Liquids

Using the densities that you calculated in Procedure 1 determine the order you will place the liquids in the 100 mL

cylinder.

In the following table, write your prediction of how the liquids should be stacked.

Fluid

Mass of Fluid and

Cylinder

Mass of Cyl-

inder

Mass of Fluid Volume of

Fluid

Density of

Fluid

Green Corn Syrup

Blue Dish Soap

Red Water

Clear Cooking Oil

Gold Honey

Liquid 5 (top)

Liquid 4

Liquid 3

Liquid 2

Liquid 1 (bottom)

IPC Lab – 1st Sixth Week—Density Column Lab

Name: _____________________

Period: _____________________


Procedure 3: Constructing Your Density Column

You will construct your density column in the 100 mL graduated cylinder. You will use the

remainder of the five fluids.

Slowly pour your predicted Liquid 1 into the cylinder.

Pour each of the remaining liquid in to the graduated cylinder in the order of the previous table.

Be sure to remember how fast each liquid pours into the cylinder.

Was your predicted density order correct? __________.

If not, what happened? __________________________________________________.

Use the flowing speed to determine the order of viscosity of the five fluids:

Procedure 4: Comparing the Density of Solids A solid placed in a liquid will float if it is less dense and sink if it is more dense.

Predict where the following six objects (penny; cork; crayon; dice; ice; aluminum foil ball)

will float in the density column.

Procedure 5: Placing the Solids in the Column Gently drop each object into the column from most to least dense.

The approximate density of the crayon must be between: _____ g/mL and ____ g/mL

Using the displacement method find the actual density of the crayon:

Mass: Volume: Density:

Did your calculation fall within your estimation of the crayon’s density?

Below draw and label the final configuration of your density column (the liquids and where the solids floated).

Greatest viscosity Least viscosity

Object 1 (floats on top)

Object 2

Object 3

Object 4

Object 5

Object 6 (sinks to bottom)

Name: _____________________

Period: _____________________


Teacher Explanation Page – (Density Column Lab)

Setup and Preparation:

Use 100 mL graduated cylinders for the density columns.

You will have to color the liquids beforehand. The colors help the students distinguish each

liquid in the column.

You may decide to have each group find the density or only one or two liquids, which can be shared with the entire

class. For each group to find each density is time consuming.

Use 10mL plastic graduated cylinders for students to measure liquid density.

Student Outcome – Write a scientific statement that explains the relationship between density and placement in the column.

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