Final Review 2013
Chapts 1-2
1. a)Hypothesis: tentative answer to a question
b) Control : used for comparison
c)Theory: explanation supported by many
experiments
d)Law: relationship in nature supported by
experiments
e) Independent Variable: one changed by the
experimenter
f) Dependent variable: one changed because
of the independent variable
Review
2a) Safety:
-goggles
-apron
-closed toe shoes
-hair tied back
Review
b)
-follow directions
-report accidents to teacher
-place waste in designated containers
-know the location of safety equipment
-no horseplay
Review
c) Flush with water for
5 minutes
d) Rinse in safety shower
(fully clothed)
Review
3. mass- electronic balance
volume- graduated cylinder
length – metric ruler
time- stop watch
temperature – thermometer
All measurements should have a NUMBER and
UNIT!
SI Units for Measurements
a)
b)
c)
d)
e)
Mass – grams
Volume – liters
Length – meter
Time – seconds
Temperature - ˚C
Accuracy & Precision
Accuratemeasurements
are CLOSE to the
accepted value
Not accuratemeasurements
are NOT CLOSE
to the accepted
value
PRECISE – series of
measurements
close to each other
Review
c) Percent error:
d) density:
e) quantitative data: numerical data (numbers)
f) qualitative data: information describing color,
odor, shape etc
Accepted value is 1.59 g/ml
Trial
Group A
Group B
Group C
1
2
3
Average
1.54
1.60
1.57
1.57
1.40
1.68
1.45
1.51
1.70
1.69
1.71
1.70
5a) Group A most accurate
b) Group C precise
c) None
% error for Group A
Trial
Group A
Group B
Group C
1
2
3
Average
1.54
1.60
1.57
1.57
1.40
1.68
1.45
1.51
1.70
1.69
1.71
1.70
5d)
(1.59 – 1.57) X 100
1.59
= 1.3%
Scientific Notation
6a) 4.5 x
10-5
=
.000045
2 sig figs
b) 8.7 x 106 = 8700000
2 sig figs
7a) 238,000 = 2.38 x 105
3 sig figs
b) 0.00072 = 7.2 x 10-4
2 sig figs
Density
8)
2100g
70mL
9)
75g
20mL
Density = 3.75g/mL
Density = 30g/mL
Density
10) 20/5 = 4g/mL
B is the same
11) Read the BOTTOM of the meniscus
Volume is 43.0mL
Graphs
13a) Pie graph- percentages b) Bar graph- comparisons
c) line graph- shows how the
dependent variable changes with a
change in the independent variable
Graphing Rules
1.
2.
3.
4.
5.
Title
Labeled axes
Equal intervals
Use up most of the page
Use a key if needed
X-axis – independent variable
Y-axis – dependent variable
Chapter 3
14) Definitions are in the textbook
a) Cutting plastic - physical
b)Rotting meat- chemical
c) water evaporating- physical
d) Dissolving salt- physical
e) Bubbles formed when vinegar reacts- chemical
f) Gold conducting electricity- physical
g) Magnesium burning- chemical
15) bubbles- chemical change ex odor, heat,
precipitate
Definitions/examples
16)Element example- Au, Zn, Br etc
Compound examples- NaCl N2O5 ZnBr2
17)
Solid
Liquid
Gas
Particles Energy Shape/vol
tight
low
definite
loose
medium def vol but
not shape
Very
high
Indefinite
loose
Homo vs Hetero
18)Salt water- homo
b)clay and oil- hetero
c) sweet tea- homo
d) kool-aid- homo
e) vegetable soup- hetero
f)chunky peanut butter- hetero
g) muddy water- hetero
Separating Substances
19)Colors in black ink- chromatography
b) salt water- evaporation
c)sand and water- filtration
d)iron filings and sulfur- magnetism
f) two different liquids- distillation
Chromatography
Filtration
Distillation
Types of Mixtures
Particles
size
Solution
tiny
Colloid
small
Suspension large
Tyndall effect
Tyndall
effect
none
yes
n/a
Settling?
no
no
yes
b is a suspension
Atomic Theory Scientists
21)USE THE TEXTBOOK – page 103 to 104
22) Use the textbook for definitions
23) See page 114 of the textbook
24) Atomic # is number of PROTONS
a) lithium atomic # 3
b) 3 protons and electrons
c) sulfur – 16 Protons
d) Lithium – 4 neutrons
25)silver-107 47 protons and 60 neutrons
26)neutrons = mass – protons = 31 neutrons
57
Fe
26
Types of Radiation
27a) Alpha
b) 4
beta
2
c)
0
0
He
gamma
ϒ
β
-1
0
Nuclear Equations
d) 226
Ra 
88
ii)
14
C 
6
222
Rn
86
14
N
7
4
He
+
2
0
β
+
-1
Fission vs Fusion
28)
• Splitting a heavy
nucleus
• Energy produced
• Fusing small nuclei
• LARGE amounts of
energy produced
• Occurs in the sun
• Responsible for all
elements heavier
than H
**Cheap source of energy with less pollution than burning
coal, however, expensive to build the plant, problems with
getting rid of nuclear waste etc
Half- Life
29)
Time
(minutes)
0
18
36
54
72
90
Amount (g)
165
82.5
41.25
20.62
10.31
5.16
Half- Life
29b)
Time
(minutes)
0
1
2
Amount (g)
10.0
5.0
2.50
Half-Life application
30) Using C-14 to determine the age of a fossil
Isotopes
31) Mg-24 contributes the most to the average
atomic mass of magnesium (closest to the
number on the periodic table), so it is the most
abundant in nature.
Weighted Average Atomic Mass
32)
Isotope
X11
X10
Mass
(amu)
10.013
11.009
%
abundance
.198
.802
Mass x %
1.9826
8.8292
TOTAL: 10.812
Element X is BORON
Chapter 5
33) Get definitions from the textbook
34) s, p, d, f
b)
Various shapes- spherical,
dumbbell etc
Sublevels
c)
SubLevel
s
p
d
f
# electrons
2
6
10
14
Electronic Configurations
35) Li- 1s22s1
b) Ne- 1s22s22p6
c) Al- 1s22s22p63s23p1
d) Ca- 1s22s22p63s23p64s2
[He] 2s1
[He] 2p6
[Ne] 3s23p1
[Ar] 4s2
36) Si
b) F
c) Na
Valence Electrons
37) Beryllium (group 2A) - 2 valence eb) Nitrogen (group 5A) - 5 valence ec) Argon- (group 8A) 8 valence ed) Sulfur- (group 6A)
6 valence ee) Boron- (group 3A)
3 valence e-
Flame Tests
38) Elements give of distinct colors when heated
in a flame. The color of the flame is matched to
the known element.
Electron Configuration
39a) 4p1 – Gallium b) 5s2 – Strontium
c) 6p6 – Radon d) 7s1 – Francium
40) Same column- similar ending config
Concepts
a) Valence e- is the SAME as the group number
a) Cesium – 1
Nitrogen – 5 Oxygen – 6
c)
Cs
N
O
d) Period tells you the # of energy levels (rings)
e) s-block (groups 1 & 2)
p-block (groups 3A-8A)
d-block (transition metals)
f-block (lanthanides & actinides)
Periodic Trends
c) Ionization Energy decreases down the group
increases across
Lowest IE – Francium
Highest IE - Helium
Periodic Trends
d) Electronegativity decreases down the group
increases across
Lowest E – Francium
Highest E - Fluorine
Periodic Trends
e) Metals become SMALLER when they turn into ions
Non-metals become LARGER
Periodic Trends
f) Francium is most active metal.
Fluorine most active non-metal.
AKS 11b Trends on Element Properties
Family
Group#
Alkali
Alkaline earth
Nitrogen grp
Carbon grp
Oxygen grp
halogens
Noble gases
Inner trans
transition
Rep elements
1A
2A
5A
4A
6A
7A
8A
f-block
d-block
A elements
#
valence
1
2
5
4
6
7
8
varies
varies
varies
charge
Examples
+1
+2
-3
+/- 4
-2
-1
0
varies
varies
varies
Li
Ca
P
Si
S
Br
Kr
U
Fe
O
AKS11b Metal/Nonmetal/Metalloid
a) Metals left, nonmetals right , metalloids
border the stairstep line. Stairstep line
separates metals and nonmetals
AKS11b Metal/Nonmetal/Metalloid
c) Metals - shiny, malleable, ductile, conduct
electricity, react with acid
Nonmetals - mostly gases, dull brittle, do not
react with acids, nonconductors
Metalloids - have properties of BOTH metals &
nonmetals
d) Metals mostly s and d block
Nonmetals and metalloids mostly p block
Chapter 8 - Ionic Bonding
1. a)
b)
CaCl2
Chapter 8 - Ionic Bonding
2a) Binary compounds – 2nd element gets “ide”
b) Roman numerals used for transition metals
that have more than one charge ex Fe2+
and Fe3+
2a) KBr - Potassium Bromide
b) CaCl2 - Calcium chloride
c) SnO2 - Tin (IV) oxide
d) Cu(NO3)2 – Copper (II) nitrate
e) Sr(OH)2 – Strontium hydroxide
Ionic Bonding question #4
Name Compound
Cation Anion
Formula
Lithium Flouride
Silver Oxide
Barium carbonate
Gold(III) sulfite
Copper (II) hydroxide
Li+
Ag+
Ba2+
Au3+
Cu2+
LiF
Ag2O
BaCO3
Al2(SO3)3
Cu(OH)2
FO2(CO3)2(SO3)2(OH)-
B or
NB
B
B
NB
NB
NB
Ionic Bonding
5a) Na2SO4 - Sodium sulfate
b) SnO2 - Tin (IV) oxide
c) FePO4 - Iron (III) phosphate
d) Ca(NO2)2 - Calcium Nitrite
e) MgCO3 - Magnesium Carbonate
f) Al(OH)3 - Aluminum hydroxide
g) (NH4)3N - Ammonium nitride
h) AgC2H3O2 - Silver acetate
i) Fe3P2 - Iron (II) phosphide
Chapt 9 - Covalent Bonding
6)
Covalent Bonding
7) Binary covalent compounds end in “ide”
9) a) PH3 - phoshporus trihydride
b) CCl4 - Carbon tetrachloride
d) NO - Nitrogen monoxide
f) As2O5 - Arsenic pentoxide
Lewis Structures
10a)
b)
c)
d)
e)
Covalent & Ionic Bonding
13 a) MgCl2 – Magnesium chloride
b) NO2 - Nitrogen dioxide
c) HF - Hydrogen fluoride
d) K3PO4 - Potassium phosphate
e) NH4Br - Ammonium bromide
f) Cu(NO3)2 – Copper (II) nitrate
Covalent or Ionic?
14b) tetraphosphorus hexoxide - P4O6
c) aluminum sulfate - Al2(SO4)3
d) Lead (IV) sulfite - Pb(SO4)2 (reduced)