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1st Sem. Final Exam Review
Honors Chemistry
_________ are substances with
constant composition that can be
broken down into elements by
chemical processes.
A) Solutions
B) Mixtures
C) Compounds
D) Quarks
E) Heterogeneous mixtures
An example of a pure substance
is
A) an element.
B) a compound.
C) pure water.
D) carbon dioxide.
E) all of these
A Classification Of
Matter
Homogeneous
Heterogeneous
Pure Substances
Elements
Atoms
Mixtures
Compounds
Nucleus
Electrons
Protons
Neutrons
Chapter 1
Structured
Overview
Chemistry
Honors Chemistry
kgm2/s2
joules
(composition, structure, & properties)
(noticed when matter changes )
Matter (possesses inertia)
work)
Energy(the ability to doFxD
Homogeneous
Heterogeneous
(uniform properties)
(uneven properties)
intensive vs. extensive chemical vs. physical
Types
Kinetic
Mixtures
Potential
(energy of
motion)
amount makes a difference
New substance formed to
notice it
Definite
PureComposition
Substances
units
(stored energy)
½ mv2
Forms
Chemical
Physical change
100% of one thing
Mechanical
No set ratio Yes!
Elements
one kind of atom No!
Heat
Property retention
Chemical change
Light
Compounds Yes!
Separation?
more than one kind of atom
(Know the techniques.) Sound
Electrical
Set ratio, Chemical blend, New properties
Physical blend
Which of the following is an example of a
qualitative observation?
A) A piece of wood is 5.3 cm long.
B) Solution 1 is much darker than
solution 2.
C) The volume of liquid in beaker A
is 4.3 mL
D) The temperature of the liquid is
60°C.
E) none of these
Express 784000000 in
scientific notation.
6
A) 7.84 x 10
8
B) 7.84 x 10
7
C) 78.4 x 10
6
D) 784 x 10
7
E) 784 x 10
Measured quantities, such as length,
mass, or time, can best be described
as:
A) sometimes certain.
B) always certain.
C) always uncertain.
D) sometimes uncertain.
A scientist obtains the number 1250.37986
on a calculator. If this number actually
has four (4) significant figures, how
should it be written?
A) 1251
B) 1250.3799
C) 1250.4
D) 1.250 x 103
E) 1.250 x 10–3
A piece of indium with a mass of 16.6 g is
submerged in 46.3 cm3 of water in a graduated
cylinder. The water level increases to 48.6 cm3.
The correct value for the density of indium from
these data is:
A) 7.217 g/cm3
B) 7.2 g/cm3
C) 0.14 g/cm3
D) 0.138 g/cm3
E) more than 0.1 g/cm3 away from any of
these values.
The SI System
Units
Fundamental
Mass, kg
Length, m
Time, s
Temp, K (°C+273)
Amount, mole
Current, A
Derived
Volume, Length3,
m3, cm3, dm3, L ,mL
(L= 1 dm3; 1 cm3= 1mL)
Density, M/V,
g/cm3
Energy, F*D, N*m
kg m2/s2 (Joule, J)
1 calorie = 4.184 J
What is the boiling point of methanol, in
Kelvins, if the temperature in centrigrade
(also called Celcius) is 66°C?
A) -207 K
B) 273 K
C) -66 K
D) 339 K
E) not enough information is given.
Foundations
Chapter 2
Structured Overview
H Chemistry
(Measurement & Calculation)
•Big Bang
•Gravity
Laws •Conservation of
•Natural
Selection
Science
Mass
Seen again and again
Observations
(Facts)
Qualitative
(Nature)
•Atomic
The Scientific Method
Hypothesis
(Explanation)
Theory
Experiments
(Tests)
Quantitative
(Measurements)
S.I. System
Scientific Notation
Write it
Units
(7)
Fundamental
Force
(F=ma)kg m/s2
percent error =
Prefixes Calculate w/ it
(9)
Derived
Dimensional
Analysis
Uncertainty
Sig
Figs
With
Precision
Meas. – True
v.
X 100%
Accuracy
True Value
devices(estimate one place)
Volume(LxLxL) dm , L,
or cm3 Zero Rules
Density (D=m/V)
3
g/cm3
Calculate with
The scientist who discovered the
charge on the electron was
A) J. J. Thomson.
B) Robert Millikan.
C) Ernest Rutherford.
D) William Thomson.
E) John Dalton.
The element rhenium (Re) exists as two
stable isotopes and 18 unstable isotopes.
Rhenium-185 has in its nucleus
A) 75 protons, 75 neutrons.
B) 75 protons, 130 neutrons.
C) 130 protons, 75 neutrons.
D) 75 protons, 110 neutrons.
E) not enough information is given.
The element magnesium (Mg) exists as
three isotopes. They are shown below with
their atomic masses and their relative
abundances:
24Mg 23.9850 amu (78.99%)
25Mg 24.9858 amu (10.00%)
26Mg 25.9826 amu (11.01%)
What is the atomic mass of magnesium on
the periodic table?
A) 23.9850 amu.
B) 24.9845 amu
C) 24.3050 amu
40Ca2+
20
has
A) 20 protons, 20 neutrons, and 18
electrons.
B) 22 protons, 20 neutrons, and 20
electrons.
C) 20 protons, 22 neutrons, and 18
electrons.
D) 22 protons, 18 neutrons, and 18
electrons.
E) 20 protons, 20 neutrons, and 22
electrons.
By knowing the number of protons a
neutral atom has, you should be able to
determine
A) the number of neutrons in the
neutral atom.
B) the number of electrons in the
neutral atom.
C) the name of the atom.
D) two of the above.
E) none of the above
If an atom of polonium (atomic number 84)
undergoes a conversion to lead (atomic
number 82) by the loss of a single particle,
A
B
C
D
the particle lost was an alpha particle
the particle lost was a gamma ray
the particle lost was a beta particle
the particle lost could have been an
alpha particle or a beta particle
E the particle lost was a positron
0.98 g Li is equal to how many moles of Li
and how many atoms of Li?
A
B
C
D
E
8.6 mol; 6.0 x 1023 atoms
0.14 mol; 8.6 x 1022 atoms
0.14 mol; 6.0 x 1023 atoms
8.6 mol; 8.6 x 1022 atoms
you can’t tell both quantities
Chapter 3... HChem.
Hard Little Spheres
History
John Dalton
Proust
Laviosier
Law of
Law of
Democritus
Definite
Conservation
______
Compostion
______
All matter
is
comprised
of atoms
Atoms of
different
elements
have
different
masses
Atoms are
indivisible
Atoms
rearrange in
chem rxtions
matter
The MOLE
Ernest Rutherford
J. J. Thomson
Planetary
Model
Gold Foil Exp.
Cathode Ray Tube Exp.
The
electron
Atomic
Theory
Use
D.A.
23
1 mole = 6.02 x 10 = molar mass
counting
them
The Atom
Plum
Pudding
model
(negatively These can be lost
or gained
charged
matter)
1.76x108 C/g
e-/m
mass of
e-
9.11x10-28 g
Element-A
nuclide
A
A particular
atom
z
X
Most are… radioactive
Atom is
mostly…
empty
Nucleons
1.6x10-19 C
Charge on
the electron
Millikan’s
________
Oil-Drop
Exp.
ratio
Nucleus
(positive,
dense
core)
Chadwick
protons
neutrons
(+ charge)
(no charge)
Atomic #
Mass #
Z
A
Mass Spec.
Atomic
isotopes Weighted
Averages
masses
Example Scenario Problem:
Barack and Michelle, graduate students at the University of Chicago in the
Metallurgy Dept., were rummaging through the supply room searching for
metals to use in their upcoming experiment. Barack found a 10.0 gram sample
of gallium in a container that had a label on it that read density = 5.91 g/cm3,
and placed it in Michelle’s hand only to find that the metal melted in her palm.
1.) When gallium melts, the change associated with the
process is
A
B
C
D
physical and endothermic
physical and exothermic
chemical and endothermic
chemical and exothermic
Example Scenario Problem:
Barack and Michelle, graduate students at the University of Chicago in the
Metallurgy Dept., were rummaging through the supply room searching for
metals to use in their upcoming experiment. Barack found a 10.0 gram sample
of gallium in a container that had a label on it that read density = 5.91 g/cm3,
and placed it in Michelle’s hand only to find that the metal melted in her palm.
3.) If Michele poured the liquid gallium into a graduated
cylinder what volume should she have found?
A
B
C
D
E
59.1 mL
0.591 mL
1.69 mL
0.0591mL
16.9 mL
Example Scenario Problem:
Barack and Michelle, graduate students at the University of Chicago in the
Metallurgy Dept., were rummaging through the supply room searching for
metals to use in their upcoming experiment. Barack found a 10.0 gram sample
of gallium in a container that had a label on it that read density = 5.91 g/cm3,
and placed it in Michelle’s hand only to find that the metal melted in her palm.
4.) If Michele poured the liquid gallium into a graduated
cylinder and actually found 1.58 mL for the volume,
what would’ve been her percent error?
A
B
C
D
E
13%
1.6 %
4.2 %
0.69 %
6.5 %
Which of the following frequencies
corresponds to light with the longest
wavelength?
13
–1
A) 3.00 x 10 s
B) 4.12 x 105 s–1
C) 8.50 x 1020 s–1
D) 9.12 x 1012 s–1
E) 3.20 x 109 s–1
What is the energy of a photon of
blue light that has a wavelength of
450 nm?
14
A) 6.7 x 10 J
B) 4.4 x 10–19 J
C) 1.5 x 105 J
D) 1.01 x 1048 J
E) 5.8 x 10–19 J
Write the electron
configuration notation for
the element Indium
2
2
6
2
6
1s 2s 2p 3s 3p 4
2
10
6
2
10
s 3d 4p 5s 4d
1
5p
Which of these elements has
three electrons in degenerate
orbitals?
A Po
B P
C Hg
D Si
E Pd
The atom does not collapse
The light emitted by atoms
For hydrogen:
(Young…Double Slit)
(What atoms have to do with it)
-1312 kJ
En= mole e- n2
Bohr Model
Sub-levels exist
Therefore
p (3) d (5)
The observer affects
the observed
Defined
If light has a dual
nature…why not matter
Schroedinger
Electrons are waves of (Max Born)
chance.
Electrons are standing waves…only
certain energies allowed
High probability regions in
as: space where the electron is
likely to be found
Filling order for atoms with more than one electron
Planck’s
Constant…
6.6x10-34J•s
What DeBroglie said
Heisenberg’s
Uncertainty Principle
(Proven by looking at
Bright-Line Spectra)
f (7)
Quantum of
energy (photon)
Wave
Mechanical
Model
These are called: orbitals
s (1)
Particle-like
E=hn
wavelength
frequency Speed of
light
electrons can have only
certain energies
colors are emitted when electrons
jump from higher to lower energy
levels
Energy levels exist
(Photo-electric effect)
(Planck / Einstein)
Wave-like
3.0 x 108m/s
lxn=c
Bright-Line Spectra
For H:
The Atom…cont’d
The Rutherford Model
could not explain…
Chapter 4 H Chem
Aufbau
Pauli
Shown with:
1.Config.
or
Hund’s
2.Orbital
Of the following elements, which
one is most likely to form an ion
through the loss of two electrons?
A sulfur
B aluminum
C sodium
D strontium
E chlorine
An element having the
1
configuration [Xe]6s belongs
to the Group:
A halogens
B None of these
C alkaline earth metals
D alkali metals
E noble gases
1. Is phosphorous a metal or nonmetal? nonmetal
2.Write the orbital notation for the
element phosphorous. 1s22s22p63s23p3
3. What is the charge on the
phosphide ion? 34. How many neutrons are in a
phosphorous atom? You can’t tell…
5. Which is bigger, the atom or the ion?
the ion!
Of the following elements, which
has the lowest first ionization
energy?
A) Ba
B) Ca
C) Si
D) P
E) Cl
Chapter 5 -- H. Chemistry
The Periodic Table
Based on
Mass
Dobereiner
Newlands
Mendeleev
left blanks
Moseley
Based on atomic
number
Reasons (based on
structure)
down
Higher Energy
Levels
Nuclear Charge
across
Terms
know the
Families “groups”
Periods
Metals/Nonmetals
“father” of the
Metalloids
periodic chart
Blocks
Isoelectronic
Valence**
←Trends
(repetition of behavior)
**outermost s and p electrons
Metallic Reactivity
Metallic Character
Atomic Size
Ionic Size
Charge
Ionization Energy
Electron Affinity
know the
transition to
these
Which of the following name(s) is (are)
correct?
1. carbon dioxide CO2
2. ammonium chloride NH4Cl
3. acetic acid HC2H3O2 (aq)
4. barium oxide BaO
A) all
B) none
C) 1, 2
D) 3, 4
E) 1, 3, 4
What is the hybridization on each oxygen
atom in a molecule of oxygen?
A)
B)
C)
D)
E)
sp
sp2
sp3
dsp3
d2sp3
Which of the following is a polar
molecule)
A) BCl3
B) SiCl4
C) PCl3
D) Cl2
E) none of these
General Properties
Soluble in water
Conductive in sol’n Chemical Bonding
Higher M.P.’s
IONIC...transfer
Electronegativity
differences
Process (steps)
Lowers
energy of system
Rationale:
Accompanied by:
I.E
E.A
L.E.
Nonconductive in sol’n
Lower M.P.’s
COVALENT...sharing
Accompanied by:
Polar Covalent…
unequal sharing
0.4-1.7
>1.7
2-D Lewis Structures
•Count
•Distribute
Insoluble in water
A Blend
^and 3-D**
• Connect
General Properties
Chapter 6 Honors Chem.
Multiple
Bonds
Exceptions to
octet rule
0.0 – 0.3
Resonance
d- d+
Polarity
of bonds
Honors
Chem.
Molecular Shapes
nonpolar
polar
(symmetrical)
(nonsymmetrical)
CH4
shows
Theory
epulsion
air
lectron
hell
alence
V S E P R
Polarity of
Molecules
(when atom arrangements vary)
**3-D Lewis
Structures
NH3
109.5° angles
possible scenarios
Example
CH4
NH3
H2O
BF3
SO2
CO2
4
3
2
3
2
2
**
# of lone pairs
0
1
2
0
1
0
resonance
(when one bonding
arrangement is insufficient)
H2O
107° angles
# of bonds**
isomerism
BF3
104.5° angle
EPA
Shape
120° angles
Hybridization
tetrahedral
tet.
sp3
tet.
trig. pyramidal
sp3
tet.
bent
sp3
trig. planar
trig. planar
<120° angle
sp2
trig. planar
bent
sp2
linear
linear
sp
Multiple bonds count the same as single bonds
SO2
180° angle