CHAPTER 3 MATTER - Mr. Pelton...

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CHAPTER 3

• Matter

• Combining Matter

• States of Matter

MATTER

Matter- Anything that takes up space (volume) and has mass.

Atom- basic unit of matter.

Subatomic particles- protons, neutrons, and electrons.

ATOM MODELS ATOMS Protons are positively charged

subatomic particles (+)

Neutrons are neutrally charged subatomic particles (no charge)

Protons and Neutrons are found in the nucleus (center) of an atom.

Protons and neutrons make up the mass of an atom (atomic mass).

ATOMS Electrons are negatively charged particles

that orbit around the nucleus.

Electrons are attracted to the nucleus and are in constant motion.

Atoms have no charge because they have equal number of protons as electrons.

(Positive) + (Negative) = No net charge

ELEMENTS

Element- a pure substance that consists

entirely of one type of atom.

There are more than 100 known elements

Elements are represented as either one or two

letters and are listed on the periodic table.

Elements are listed on the periodic table by the

number of protons/electrons that they have.

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SYMBOLS FOR ELEMENTS

All elements are classified and arranged

according to their chemical properties in the

periodic table of elements.

The number of protons and neutrons in atoms

of different elements varies widely.

Atomic number is the number of protons in an

atoms nucleus.

Atomic mass = # Protons + # Neutrons

VALENCE ELECTRONS

The electrons in the outermost energy level determine the chemical behavior of the different elements.

The outermost electrons are called valence electrons

HOW MANY VALENCE ELECTRONS DOES

CARBON HAVE? IDENTIFYING ATOMS

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IDENTIFYING ATOMS IDENTIFYING ATOMS

IDENTIFYING ATOMS ELECTRONS

Electrons occupy areas around the nucleus of an atom called energy levels

The innermost energy level can only hold 2 electrons.

The second energy level is larger, it can hold up to 8 electrons.

ISOTOPES

Isotopes- atoms of an element that have different number of neutrons.

Isotopes have a different atomic mass, but the same atomic number.

Because they have the same number of electrons, all isotopes of an element have the same chemical properties.

Radioactive isotopes- have unstable nuclei that break down at a constant rate over time, and are used for dating purposes, and tracers.

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ISOTOPES OF CARBON IONS

• An atom that loses electrons

becomes positively charged (+)

• An atom that gains electrons

becomes negatively charged (-)

• Positively and negatively charged

atoms are called IONS

• Ions are atoms that either gain or

lose electrons

VOCABULARY:

Matter:

Element:

Nucleus:

Proton:

anything that takes up space (volume) and has mass.

a pure substance that consists entirely

of one type of atom.

the center of the atom which contains the protons and neutrons

positively charged particles that make up the nucleus of an atom

VOCABULARY:

Neutron:

Electron:

Atomic

Number:

Atomic

Mass:

particles found in the nucleus of an atom that have no charge.

negatively charged particles that orbit

around the nucleus.

the number of protons in an atoms

nucleus.

# Protons + # Neutrons

VOCABULARY:

Isotopes:

Ions:

Atoms of the same element that have a different number of neutrons (different atomic mass).

An atom which gains or loses an electron

and has a net electric charge

CHEMICAL COMPOUNDS

Most elements in nature are found combined with other elements.

Compound- a substance formed by the chemical combination of two or more elements in specific proportions.

Chemical formula- the composition of compounds in terms of types of elements, and numbers of each.

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CHEMICAL BONDS CONTINUED

Molecule- the smallest unit of most compounds (ex. H20)

Molecules have no overall electric charge.

Molecules form covalent bonds

CHEMICAL COMPOUNDS

Examples of compounds and chemical formulas. H2O CO2 C6H12O6

NaCl HCl

CHEMICAL COMPOUNDS

NaCl = Sodium Chloride = Table Salt

Combination of sodium and chlorine

CHEMICAL BONDS

Atoms in compounds are held together by chemical bonds.

Ions – atoms that lose or gain electrons

Ionic bond- is formed when one or more electrons are transferred from one atom to another (ex. NaCl).

IONIC BOND CHEMICAL BONDS CONTINUED

Covalent bond- situation where elements share electrons between them, instead of transferring them.

Electrons travel in the energy levels of both atoms in a covalent bond.

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CHEMICAL BONDS CONTINUED

Metallic bond- valence electrons are shared between all atoms.

Electrons “flow” through metals

This “flow” allows metals to conduct electricity.

METALLIC BOND

Valence electrons move

freely around positively

charged ions of the

metal.

CHEMICAL REACTIONS:

The change of one or more substance into another substance is called a chemical reaction.

Bonds holding atoms together are rearranged during a chemical reaction: Ex: H2 + O2 → H2O Fe + O2 → Fe2O3

Reactant + Reactant → Product

PHOTOSYNTHESIS

CO2 + H2O → C6H12O6 + O2

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DRAWING MOLECULES SOLUTIONS AND SUSPENSIONS

Mixtures- a combination of two or more components that retain their identities. Ex: cinnamon and sugar, salt water

Solution- a mixture in which one or more substances are uniformly distributed in another substance. Ex: Seawater, air, kool-aid

ACIDS AND BASES

Acid: a solution containing a substance that produces hydrogen ions (H+) in water.

Base: a substance that produces

hydroxide ions (0H-) in water.

Neutral: a solution which has equal proportions of H+ and 0H- ions in water.

ACID

BASE

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pH SCALE

The pH scale is a measure of

how acidic or basic a

substance is. It directly

measures the concentration of

H+ ions in solution.

CHEMICAL COMPOUNDS


Compound- a substance formed by the chemical combination of two or more elements in definite proportions.


PROPERTIES OF WATER

Water covers over 75% of the Earth’s surface.

Water is the single most abundant compound

in most living things.

It is a liquid at most of Earth’s temperatures.

It expands when it freezes and is less dense

than liquid water.

It is neutral in charge, but polar.

Polarity- an uneven distribution of electrons.

PROPERTIES OF WATER

Water is the universal solvent because it dissolves more substances than any other liquid.

Pure water is 7.0 on the pH scale (Neutral).

Water moves against the force of gravity due to capillary action.

Water has a high surface tension and a high specific heat index.

CHEMICAL COMPOUNDS




http://globe.gsfc.nasa.gov/cgi-bin/home.cgi

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CHEMICAL COMPOUNDS

Examples of compounds and chemical formulas H2O CO2 C6H12O6

NaCl HCl

CHEMICAL COMPOUNDS



SOLUTIONS AND SUSPENSIONS

Mixtures- a material composed of two or more elements or compounds that are physically mixed together but not chemically combined.

Solution- a mixture in which one or more substances are uniformly distributed in another substance.

Solutions can be a liquid, solid, or gas, or any combination.

BELL RINGER Draw the Bohr model of the

following atoms:

Hydrogen

Carbon

Nitrogen

Oxygen

HYDROGEN CARBON

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NITROGEN OXYGEN

VALENCE ELECTRONS

The electrons in the outermost energy level determine the chemical behavior of the different elements.

The outermost electrons are called valence electrons

HOW MANY VALENCE ELECTRONS?

Hydrogen?

Carbon?

Nitrogen?

Oxygen?

ISOTOPES

Isotopes- atoms of an element that have different number of neutrons.

ISOTOPES OF CARBON

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CHEMICAL COMPOUNDS




CHEMICAL COMPOUNDS

Examples of compounds and chemical formulas H2O CO2 C6H12O6

NaCl HCl

CHEMICAL COMPOUNDS



VOCABULARY:

Matter:

Element:

Nucleus:

Proton:

anything that takes up space (volume) and has mass.

a pure substance that consists entirely

of one type of atom.

the center of the atom which contains the protons and neutrons

positively charged particles that make up the nucleus of an atom

VOCABULARY:

Neutron:

Electron:

Atomic

Number:

Atomic

Mass:

particles found in the nucleus of an atom that have no charge.

negatively charged particles that orbit

around the nucleus.

the number of protons in an atoms

nucleus.

# Protons + # Neutrons

VOCABULARY:

Isotopes:

Ions:

Atoms of the same element that have a different number of neutrons (different atomic mass).

An atom which gains or loses an electron

and has a net electric charge

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CHEMICAL FORMULAS

Carbon is written first if it is

present in the molecule.

Oxygen is written at the end of

the formula.

Hydrogen is written directly after

carbon if both are present.

CHEMICAL BONDING

Hydrogen can make 1 bond (1 V.E.)

Carbon can make 4 bonds (4 V.E.)

Nitrogen can make 3 bonds (5 V.E.)

Oxygen can make 2 bonds (6 V.E.)

BUILDING MODELS

H2O

BUILDING MODELS

CO2

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BUILDING MODELS

NH3

BUILDING MODELS

C2H2

BUILDING MODELS

CH4

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BUILDING MODELS

C3H8

CHEMICAL REACTIONS

Atoms can combine to form

compounds, or break down into

simpler substances.

Matter cannot be created or

destroyed

The number of atoms that enter a

chemical reaction are equal to the

number of atoms after the chemical

reaction.

CHEMICAL REACTIONS

• Chemical reaction- a process that changes one set of chemicals into another set of chemicals.

• Reactants- elements or compounds that enter a reaction.

• Products- elements or compounds that are produced by a chemical reaction.

CHEMICAL REACTIONS

Chemical reactions must be balanced since matter cannot be created or destroyed.

This is called “The law of conservation of matter”.

A chemical equation is a short-hand

way of writing a chemical reaction.

Reactants are on the left of the

equation. Products are on the right.

Mg + 2HCl MgCl2 + H2

reactants products

WHAT IS A CHEMICAL EQUATION?

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CHEMICAL REACTIONS

Atoms are not CREATED or DESTROYED

during a chemical reaction. Scientists know

that there must be the SAME number of

atoms on each SIDE of the EQUATION. To

balance the chemical equation, you must

add COEFFICIENTS in front of the chemical

formulas in the equation. You cannot ADD

or CHANGE subscripts!

BELL-RINGER

Balance the following equations.

__H2 + __O2 → __H2O

__CO+ __O2 → __CO2

REVIEW QUESTIONS (3.1)

1. Differentiate among the three parts of an atom in terms of their location, charge, and mass.

2. Explain why the elements magnesium and calcium have similar properties.

3. How does a neutral atom become an ion?


4. Compare and contrast these isotopes: uranium-239 uranium-238 uranium-235

5. Draw a model of a calcium atom, including the number and position of protons, neutrons, and electrons in the atom.

6. Why is the atomic mass of most elements not a whole number?


7. As the radioactive isotope radium-266 decays, it

emits two protons and two neutrons. How many

protons and neutrons are now left in the nucleus?

What is the atom’s new atomic number? What is the

name of this element?

86 protons

136 neutrons

Atomic number = 86 = radon.


1. Explain why molecules do not have electric

charges.

2. Differentiate between molecules and

compounds.

3. (Skip)

4. How can an acid be neutralized?

5. Compare and contrast mixtures and solutions

(all compounds are molecules, but not all

molecules are compounds)

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BELL RINGER: What is the chemical formula

for water?

What does the chemical

formula represent?

What is the difference between

frozen water and liquid water?

SECTION 3.3: STATES OF MATTER

All matter on Earth and

in the universe occurs in

the form of a solid, a

liquid, a gas, or plasma.

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SOLIDS

Solids are substances with densely

packed particles, which can be ions,

atoms, or molecules.

Most solids are crystalline structures

because the particles of a solid are

arranged in regular geometric

patterns.

CRYSTALLINE STRUCTURE OF DIAMOND

SOLIDS

Some solid materials have no regular

internal patterns.

Glass is a solid that consists of

densely packed atoms arranged

randomly.

Glass does not form crystals.

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LIQUIDS

At any temperature above absolute

zero (-273° C), the atoms in a solid

vibrate.

Vibrations increase with increasing

temperature (thermal vibrations)

At melting point, vibrations become

vigorous enough to break the forces

holding the solid together.

LIQUIDS

Liquids take the shape of

their container

Liquids also have a definite

volume.

GASES

The particles in liquid move and

vibrate vigorously. Some particles

gain enough energy to escape the

liquid.

The process from changing from a

liquid to a gas is called evaporation.

When any liquid reaches its boiling

point, it vaporizes quickly as a gas.

PLASMA

When a gas is heated to a

temperature of 5000°C, particles are

so violent that electrons are knocked

away from atoms and give off light.

The gases of stars, lightning, and

neon signs are all examples of matter

in a plasma state.

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CHANGES OF STATE

When some solids are heated, they

become liquid in a process called

melting

When a liquid is heated to the boiling

point, it absorbs enough thermal

energy to evaporate and become a

gas.

CHANGES OF STATE

When a gas is cooled, it

becomes a liquid in a process

called condensation

A change of state from a solid

into a gas is called sublimation.

CHAPTER 3 REVIEW

• The positively charged particle in an

atom is called the:

A. neutron

B. ion

C. proton

D. electron

CHAPTER 3 REVIEW

• The positively charged particle in an

atom is called the:

A. neutron

B. ion

C. proton

D. electron

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CHAPTER 3 REVIEW

• The electrically neutral particle in an

atom are called __________

A. neutrons

B. ions

C. protons

D. electrons

CHAPTER 3 REVIEW

• The electrically neutral particle in an

atom are called __________

A. neutrons

B. ions

C. protons

D. electrons

CHAPTER 3 REVIEW

• The atomic mass of an atom is equal

to the sum of the

A. protons and electrons

B. neutrons and electrons

C. protons and neutrons

D. protons only

CHAPTER 3 REVIEW

• The atomic mass of an atom is equal

to the sum of the

A. protons and electrons

B. neutrons and electrons

C. protons and neutrons

D. protons only

CHAPTER 3 REVIEW

• Atoms of an element that differ by

their mass number are called

A. ions

B. isotopes

C. compounds

D. bosons

CHAPTER 3 REVIEW

• Atoms of an element that differ by

their mass number are called

A. ions

B. isotopes

C. compounds

D. bosons

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CHAPTER 3 REVIEW

• What is the atomic number of this

atom?

A. 3

B. 4

C. 5

D. 6

CHAPTER 3 REVIEW

• What is the atomic number of this

atom?

A. 3

B. 4

C. 5

D. 6

CHAPTER 3 REVIEW

• How many valence electrons does

this atom have?

A. 1

B. 2

C. 3

D. 4

CHAPTER 3 REVIEW

• How many valence electrons does

this atom have?

A. 1

B. 2

C. 3

D. 4

CHAPTER 3 REVIEW

• Which element does this atom

represent?

A. He

B. Be

C. Li

D. N

CHAPTER 3 REVIEW

• Which element does this atom

represent?

A. He

B. Be

C. Li

D. N

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CHAPTER 3 REVIEW

• The figure shows the arrangement of atoms in a substance. What is this substance? A. gas B. glass C. liquid D. solid

CHAPTER 3 REVIEW

• The figure shows the arrangement of atoms in a substance. What is this substance? A. gas B. glass C. liquid D. solid

CHAPTER 3 REVIEW

• What kind of ion is characteristic of

an acid?

A. oxygen ion

B. negative ion

C. hydroxide ion

D. hydrogen ion

CHAPTER 3 REVIEW

• What kind of ion is characteristic of

an acid?

A. oxygen ion

B. negative ion

C. hydroxide ion

D. hydrogen ion

CHAPTER 3 REVIEW

• During the process of sublimation,

ice is converted into___________.

A. hydrogen and hydroxide ions

B. hydrogen

C. liquid water

D. water vapor

CHAPTER 3 REVIEW

• During the process of sublimation,

ice is converted into___________.

A. hydrogen and hydroxide ions

B. hydrogen

C. liquid water

D. water vapor

CHAPTER 3 MATTER - Mr. Pelton...

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