First Semester Review

1
First Semester Review

• Units I - IX

2
Unit IMeasurement

• You are responsible for lab safety, techniques
  equipment!

• Numerical data is called ____________ data.

quantitative

• Descriptive data is called ____________ data.

qualitative

• The amount of matter an object contains is known
  as _____.

mass

• The effect of gravity pulling on mass is known
  as ________.

weight

• How close measurements are to each other
  (consistency) is known as
  __________.

precision

• How close measurements are to being correct is
  known as __________.

accuracy
3
Unit IMeasurement

• Label the following as accurate or precise

Accurate
Precise
Neither

• Give the following S.I. Units

second (s)

• Time

• Length

meter (m)

• Volume

joule (J)
cubic meter (m3)

• Energy

• Mass

kilogram (kg)

• Temperature

Kelvin (K)
gram per milliliter (g/mL)

• Density

4
Unit IMeasurement

• How many significant digits

4 sig. digs.

• 152600000

• 320000.056

9 sig. digs.

• 0.0000569000

6 sig. digs.

• How many significant digits in your answer

2 sig. digs.

• 1.234x1012 x 3.26 x 2.0x106

1 sig. dig.

• 3000 4.56x10-4

• Put the following in scientific notation

6.023 x 1013

• 60230000000000

5.23 x 10-6

• 0.00000523

5
Unit IMeasurement

• Fill in the following chart about the metric
  system

Prefix
Sci. Not.
Factor
Symbol
1000
103
kilo-
k
hecto-
102
h
100
da
10
deka-
101
liter, meter or gram
Base Unit-
100
1
deci-
10-1
d
.1
c
.01
centi-
10-2
m
milli-
.001
10-3
6
Unit IMeasurement
Solve the following DA problems
How many minutes are in 27.4 years?
27.4 years
24 hours
60 minutes
365.25 days
1 year
1 day
1 hour
How many pounds are in 6.84 x 1015 milligrams?
1 pound
1 gram
6.84 x 1015 mg
1000 mg
454 grams
7
Unit IIAtomic Structure
Daltons Atomic Theory

• All matter is made of tiny, indivisible particles
  (atoms)

• Atoms of the same element are identical and
  unique from any other element.

• Atoms of diff. elements can physically mix
  together or can chemically combine to form
  compounds

• Chemical rxns. occur when atoms are separated,
  joined, or rearranged. However, atoms of one
  element are never changed into another element

Three subatomic particles
protons (p),
neutrons (n0)
and electrons (e-)

• Protons carry a ____________ charge.

positive

• Neutrons carry a ____________ charge.

neutral
negative

• Electrons carry a ____________ charge.

• Protons and neutrons are located in the
  ____________.

nucleus

• Electrons are located in the ______________.

electron cloud
8
Unit IIAtomic Structure
Element
Phosphorus
Atomic Mass
31 a.m.u.
Atomic
15
of protons
15
of neutrons
16
14
of electrons
Atomic Mass
55 a.m.u.
Atomic
25
of protons
25
Manganese - 55
of neutrons
30
of electrons
25
Atomic symbol
9
Unit IIAtomic Structure
Which of the following are isotopes
1 and 2 are isotopes!
Radioactive Decay
Gamma radiation
Beta decay
Alpha decay
10
Unit IIAtomic Structure
Which decay is described below
alpha decay

• same as helium nucleus

• comes from the breakdown of a neutron

beta decay

• most penetrating

gamma radiation

• most damaging

alpha decay

• least penetrating

alpha decay
gamma radiation

• least damaging

beta decay

• increases atomic number by one

• decreases atomic number by two

alpha decay
11
Unit IIAtomic Structure
Balance and label the following transmutation
reaction
Target nucleus
Ejected particle
Projectile
Product
Fission or fusion

• creates more energy

fusion

• used on the sun

fusion

• used in power plants

fission

• splits a large nucleus with a neutron

fission

• combines different atoms into one nucleus

fusion
Half-Life

• 1000 grams of substance has a ½ life of 30
  years. How much will be left after 150 years?

31.25 grams
12
Unit IIIelectronic Structure
rainbow

• When light travels through a prism, a
  ___________ appears.

• A long wavelength will have a (high / low)
  frequency. This is a(n) ___________
  relationship.

inverse
inverse

• A low frequency has (high / low) energy. This
  is a(n) ___________ relationship.

• When an atom absorbs energy, an electron will
  jump up to the __________ state and will then
  fall back down to its ___________ state.

excited
ground

• In order to fall from the excited state to the
  ground state, the electron must emit energythis
  energy is in the form of __________.

light
13
Unit IIIelectronic Structure

• The four quantum numbers are

(principle) energy level
- n
shape of cloud
- l
orientation in space
- m
- s
spin of electron

• The four sub-orbitals are

sphere
2
1
s
6
dumbbell
p
3
10
5
d
cloverleaf
14
7
too complicated
f
14
Unit IIIelectronic Structure

• What is the maximum of electrons that can fill
  the 4th energy level?

2n2 2(4)2
32

• Indicate the electron configuration, pictorial
  notation and electron dot structure for BROMINE
  (Z 35)

Electron Configuration
4s2
3d10
4p5
1s2
2s2
2p6
3s2
3p6
Pictorial Notation (highest energy level)
Electron Dot Structure
Br
15
Unit IVPeriodicity
Mendeleev

• The first periodic table was designed by
  __________ and was arranged in order of
  increasing atomic ________.

mass
Moseley

• The modern periodic table was designed by
  __________ and is arranged in order of increasing
  atomic ________.

number
periods

• Horizontal rows on the periodic table are called
  ________ and represent _______________.

energy levels
groups / families

• Vertical columns on the periodic table are
  called ________________ and represent
  __________________.

valence electrons
eight

• According to the octet rule, all atoms (except H
  and He) need ________ valence electrons to be
  stable.

two
two

• Calcium has _______ valence electrons and needs
  to (lose / gain) ______ electrons to become
  stable. Therefore, its oxidation is _______.

2
five
three

• Nitrogen has _______ valence electrons and needs
  to (lose / gain) ______ electrons to become
  stable. Therefore, its oxidation is _____.

- 3
16
Unit IVPeriodicity

• Label the following periodic table

1A
Metalloids
8A
2A
7A
BGroups
Alkali Metals
Halogens
Noble Gases
Alkaline Earth Metals
Transition Metals
Rare Earth Metals
Lanthanide Series
Actinide Series
17
Unit IVPeriodicity

• What is the outer electron configuration for
  Barium (Z 56)?

6s2

• What element has the outer electron
  configuration of 5s2 5p5?

Iodine

• The distance between the nucleus of an atom and
  its valence electrons is known as _________
  _________.

atomic
radius

• Atomic radius increases as you move

18
Unit IVPeriodicity

• The distance between the nucleus of an atom and
  its valence electrons after the atom has gained
  or lost electrons is known as _______ _______.

ionic
radius

• Ionic radius increases as you move

cations
anions

• The energy needed to steal an electron away from
  an atom is known as ___________ ___________.

ionization
energy

• Ionization energy increases as you move

19
Unit IVPeriodicity

• The tendency to attract unshared electrons is
  known as _______________.

electronegativity

• Electronegativity increases as you move

metallic

• The tendency of an atom to lose electrons is
  known as ___________ _________.

character

• Metallic character increases as you move

20
Unit IVPeriodicity
non-metallic

• The tendency of an atom to gain electrons is
  known as ______________ _________.

character

• Non-metallic character increases as you move

21
Unit VNomenclature

• Metals tend to (lose / gain) electrons to have a
  ( / - ) charge and therefore, they
  are called _________.

cations

• Non-metals tend to (lose / gain) electrons to
  have a ( / - ) charge and therefore,
  they are called _________.

anions

• Label the following compounds as either binary
  ionic, binary molecular, binary acid, ternary
  ionic or ternary acid

• Al2(SO4)3

ternary ionic
aluminum
sulfate

• NO2

binary molecular
dioxide
nitrogen

• HF

binary acid
hydrofluoric
acid

• Na2S

binary ionic
sodium
sulfide

• HC2H3O2

ternary acid
acetic
acid

• Name the compounds above

22
Unit VNomenclature

• Write the formula for the following compounds

• iron III nitrate

Fe(NO3)3

• hydroiodic acid

HI
CCl4

• carbon tetrachloride

• carbonic acid

H2CO3

• stannous oxide

SnO

• A compound in which the ratio of A to B is 3 to
  2 would have a chemical formula of __________.

A3B2

• If the compound above has a total mass of 40.
  grams, how much A and B would there be?

3X 2X 40
A 24 grams
B 16 grams
23
Unit VIBonding
ionic
bond

• The type of bond in which electrons are
  transferred is ________ _______.

polar

• The type of bond in which electrons are
  unequally shared is ________ __________.

covalent
pure

• The type of bond in which electrons are equally
  shared is ________ __________.

covalent
metallic
bond

• The type of bond that contains delocalized
  electrons is ________ ______.

• Delocalized electrons give metals what three
  unique properties

can be hammered

• malleable

• ductile

can be drawn into a wire

• good electrical conductor

24
Unit VIBonding

• Fill in the following table

Pure Covalent
gases
low
.4
weakest
Polar Covalent
Soft solids and liquids
medium
.4 - 1.66
medium
crystalline solids
strongest
Ionic
high
1.67
25
Unit VIBonding

• The forces that hold atoms together in a
  compound are known as (intermolecular /
  intramolecular) bonds.

• The forces that holds groups of compounds
  together are known as (intermolecular /
  intramolecular) attractions.

• The three intermolecular attractions are

only seen in diatomic halogens

• dispersion forces

• dipole interactions

() end of one dipole attracted to () end of a
different dipole

• hydrogen bonds

Hydrogen strongly attracted to an electronegative
atom (N, O, or F)
s

• Hybridization allows atoms to create more bonds
  by promoting a(n) ____ electron to a _____
  orbital.

p
26
Unit VIBonding

• What three groups will undergo hybridization?

Groups IIA,
IIIA and
IVA

• Draw the electron dot structure of NH3 and
  indicate whether it is a polar or non-polar
  molecule.

x
x
N
x
x
POLAR
x

• Draw the electron dot structure of AlCl3 and
  indicate whether it is a polar or non-polar
  molecule.

Al
x
x
NON-POLAR
x