Post on 29-Dec-2015
Bellwork Fri. Sept. 7
On your bellwork sheet write “Bill Nye” and on a separate sheet of paper copy down the following:
• All matter is made of ________ which are so small we can't even see them with a microscope.
• Tiny _____________ orbit the nucleus. • Atoms are like letters and when combined they make
______________which are like words.• Different materials have unique atoms. It is the number of
______________ in the nucleus that makes each materials atom unique.• ______________is a fundamental building block of all life on our planet.
It is so important it has its own entire branch of chemistry - organic chemistry.
::
Bellwork, Mon. Sept 10
In a scientific experiment, which variable is the one that is manipulated (changed) by the experimenter?
Bellwork, Tues. Sept 11
Name the 3 atomic particles & list their respective charges.
**Don’t forget to pick up a sheet off my lab bench. Have out your periodic table**
Bellwork, Wed. Sept 12
How many protons, neutrons & electrons are in a neutral atom of Calcium?
**Don’t forget to have out the story on the back of your periodic table and your atom drawings from yesterday**
Bellwork, Thurs. Sept 13
Name 5 elements that you already know.
**Don’t forget to pick up a sheet off my lab bench. Have out your periodic table**
Bellwork, Fri. Sept. 14
Which element is LEAST likely to combine with another element to form a molecule?
- Chlorine (Cl), a halogen- Iron (Fe), a metal- Neon (Ne), a noble gas- Silicon (Si), a metalloid
Bellwork, Mon. Sept. 17
The element silicon is best used for which purpose?
- as a container to keep coffee hot
- as a semiconductor in a computer chip
- as a material to make airplane frames
- as a malleable material for coins and jewelry
**I am stamping Atomic Math work from Friday**
Bell Work, Tues. Sept. 18
How can a scientist, using the periodic table, find an element with properties similar to another element?
- by comparing density - by finding it’s periodic group - by comparing malleability - by comparing atomic weight
Atom
ATOMS, are the basic particle from which all matter is made. They are so small they cannot be seen even with a microscope.
Elements ELEMENTS are one or
more identical ATOMS and each element has its own unique atom that looks different than all the other elements.
Examples
An ELEMENT is a pure substance that cannot be broken down into any other substance by chemical or physical means.
Such as:
•aluminum
•zinc
•oxygen
Subatomic Particles
Each element’s atom is unique due to the number of each subatomic particle that it contains.
Nucleus contains:• Protons – positive + charge• Neutrons – neutral / no charge Orbiting the nucleus are:• Electrons – negative - charge
The Periodic Table
The PERIODIC TABLE contains information about all the different ELEMENTS.
Natural vs. Synthetic
The majority of the known elements are naturally occurring, however all elements above 92, are SYNTHETIC meaning they were created in a lab.
Protons (+)
Elements are organized on the periodic table by their ATOMIC NUMBER, which is the number of PROTONS (+) in the nucleus.
Electrons (-)
One of an atom’s main goals in life is to remain neutral. Since protons have a positive charge, it would need to have the same number of negative charges (electrons) to remain neutral. The ATOMIC NUMBER, therefore tells us the number of electrons in a neutral atom as well.
5 Positive + -5 Negative = 0 Neutral
Isotopes Atoms of the same element
can have different numbers of NEUTRONS; the different possible versions of which are called ISOTOPES.
Atomic Mass
The ATOMIC MASS listed
on the periodic table is an average of the mass of all known isotopes of that element.
You can also think of it as the number of PROTONS and NEUTRONS.
Neutrons
Round the atomic mass to the nearest whole number and subtract the atomic #
Ex: K 39 – 19 = 20 neutrons.
Symbols
Hg – Mercury Au – Gold Pb – Lead Sn – Tin Ag – Silver Cu – Copper Fe – Iron K – Potassium Na - Sodium
Black = Solid Blue = Liquid Red = Gas
Energy Levels
There are up to seven ENERGY LEVELS within the electron cloud on which the electrons orbit the nucleus.
The PERIOD (row) on which an element can be found will tell you how many energy levels there are in an atom of that element.
Electron Configurations
1st energy level holds 2 electrons
2nd energy level holds 8 electrons
3rd energy level holds 18 electrons
Valence Electrons
The electrons that reside in the outermost energy level are the only ones involved in chemical bonding and they are called VALENCE ELECTRONS.
You can find out at a glance how many valence electrons an element has by looking at the GROUP NUMBER.
Groups / Families
• Elements in the same GROUP / FAMILY (column) have similar properties.
• The groups are numbered 1 – 18 from left to right and are typically named after the first element at the top of the group.
• Some groups have other names they are known by however:
Group 1
ALKALI METALS – do not occur uncombined in nature and are HIGHLY chemically reactive
Alkali MetalsH
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Group 2
ALKALINE EARTH METALS – also do not occur uncombined; good conductors
Alkaline Earth MetalsH
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Groups 3-12
Transition Metals – also good conductors; form colorful compounds that last a long time since they are not super chemically reactive.
Rare Earth Metals
Lanthanides
• Soft, shiny, malleable metals with high conductivity.
• Found in a lot of superconductors and laser technology.
Lanthanide SeriesH
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
La
Actinides
• They are radioactive!• Many are synthetic meaning
the nuclei are unstable (they break apart easily).
Actinide SeriesH
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
La
Ac
Metalloids
Along the stair step line – (7) METALLOIDS that have
properties of metals and non-metals are very useful. Especially for their varying abilities to conduct electricity (i.e. SILICON silicon semi-conductors in computer chips).
Non-Metals
The NON-METALS are not good conductors but they combine with others readily to form compounds.
Many of these elements are crucial in creating and maintaining life (C H N O P S).
Group 17
HALOGENS - meaning “salt forming” Form salts when combined with Alkali Metals
They are DIATOMIC,
meaning they never exist as a single atom.
HalogensH
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
**Notice that this is the only family in which the members come in all normal phases**
Diatomic ElementsH2
N2 O2 F2
Cl2
Br2
I2
Tl At
S
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Pb Bi Po
Al Si P
B C
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
S
Tl
Group 18
NOBLE GASES – do not react with other elements.
They are noble, they don’t
mix with commoners.
They are all gases at normal phase (room temperature).
Noble GasesH
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Metallic Characteristicmetallic character increases
nonmetallic character increases
met
allic
cha
ract
er in
crea
ses
non
met
allic
cha
ract
er in
crea
ses
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
K
19
Ca
20
Sc
21
Ti
22
V
23
Cr
24
Mn
25
Fe
26
Co
27
Ni
28
Cu
29
Zn
30
Ga
31
Ge
32
As
33
Se
34
Br
35
Kr
36
Rb
37
Sr
38
Y
39
Zr
40
Nb
41
Mo
42
Tc
43
Ru
44
Rh
45
Pd
46
Ag
47
Cd
48
In
49
Sn
50
Sb
51
Te
52
I
53
Xe
54
Cs
55
Ba
56
Hf
72
Ta
73
W
74
Re
75
Os
76
Ir
77
Pt
78
Au
79
Hg
80
Tl
81
Pb
82
Bi
83
Po
84
At
85
Rn
86
Fr
87
Ra
88
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
Ce
58
Pr
59
Nd
60
Pm
61
Sm
62
Eu
63
Gd
64
Tb
65
Dy
66
Ho
67
Er
68
Tm
69
Yb
70
Lu
71
Th
90
Pa
91
U
92
Np
93
Pu
94
Am
95
Cm
96
Bk
97
Cf
98
Es
99
Fm
100
Md
101
No
102
Lr
103
La
57
Ac
89
1
2
3
4
5
6
7
METALS
Nonmetals
Metalloids
Metals and Nonmetals
Properties
• A PROPERTY is a characteristic of a substance that can be observed.
• A PHYSICAL PROPERTY is one that can be observed without changing the substance.
• A CHEMICAL PROPERTY can only be observed while changing the substance.
Physical Properties• Malleability - the ability to be hammered into a
thin sheet
• Ductility - the ability to be stretched into a wire
• Melting/Freezing/Boiling point – temperature at which phase change occurs
• Density – the amount of matter in a given volume D=m/v
• Solubility – ability to dissolve in another substance
• Specific heat - the amount of heat required to heat a substance 1 degree Celsius
• Luster - shiny, dull