1. 1st Sem. Final Exam Review
Honors Chemistry

2. _________ 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

3. An example of a pure substance is
A) an element.
B) a compound.
C) pure water.
D) carbon dioxide.
E) all of these

4. Matter A Classification Of Homogeneous Heterogeneous Pure Substances
Mixtures
Elements
Compounds
Nucleus
Protons
Atoms
Electrons
Neutrons

5. Chemistry Matter Energy Kinetic Potential ½ mv2 Pure Substances
Chapter 1 Structured Overview
Chemistry
Honors Chemistry
kgm2/s2
(composition, structure, & properties)
(noticed when matter changes )
joules
Matter
Energy
(possesses inertia)
(the ability to do work)
FxD
units
Types
Homogeneous
Heterogeneous
(uniform properties)
(uneven properties)
Kinetic
Potential
intensive vs. extensive
chemical vs. physical
(energy of motion)
(stored energy)
amount makes a difference
New substance formed to notice it
½ mv2
Pure Substances
Definite Composition
Forms
Mixtures
Chemical
Physical blend
No set ratio
Property retention
Physical change
100% of one thing
Mechanical
Elements
Yes!
No!
one kind of atom
Heat
Chemical change
Light
Compounds
Separation?
Yes!
Sound
more than one kind of atom
(Know the techniques.)
Electrical
Set ratio, Chemical blend, New properties

6. 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

7. Express 784000000 in scientific notation.
A) 7.84 x 106
B) 7.84 x 108
C) 78.4 x 107
D) 784 x 106
E) 784 x 107

8. 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.

9. A scientist obtains the number 1250. 37986 on a calculator
A scientist obtains the number on a calculator. If this number actually has four (4) significant figures, how should it be written?
A) 1251 B) C)
D) x 103
E) x 10–3

10. A piece of indium with a mass of 16. 6 g is submerged in 46
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) g/cm3
B) 7.2 g/cm3
C) 0.14 g/cm3
D) g/cm3
E) more than 0.1 g/cm3 away from any of
these values.

11. Units The SI System Fundamental Derived Mass, kg
Volume, Length3, m3, cm3, dm3, L ,mL
Length, m
(L= 1 dm3; 1 cm3= 1mL)
Time, s
Density, M/V, g/cm3
Temp, K (°C+273)
Energy, F*D, N*m kg m2/s2 (Joule, J)
Amount, mole
Current, A
1 calorie = J

12. 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.

13. Foundations (Measurement & Calculation)
Chapter Structured Overview
H Chemistry
Big Bang
Natural Selection
Atomic
Gravity
Conservation of Mass
Laws
Science
Seen again and again
The Scientific Method
Theory
Observations
Grand
(Facts)
Hypothesis
Experiments
(Explanation)
(Tests)
Qualitative
Quantitative
(Nature)
(Measurements)
Dimensional Analysis
S.I. System
Scientific Notation
Uncertainty
Write it
percent error =
Meas. – True
True Value
Precision v. Accuracy
Units
Prefixes
Calculate w/ it
Sig Figs
(9)
X 100%
(7)
Fundamental
Derived
With devices
(estimate one place)
dm3, L, or cm3
Volume
(LxLxL)
Force
Zero Rules
Density
(D=m/V)
(F=ma)
kg m/s2
Calculate with
g/cm3

14. 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.

15. 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.

16. The element magnesium (Mg) exists as three isotopes
The element magnesium (Mg) exists as three isotopes. They are shown below with their atomic masses and their relative abundances:
24Mg amu (78.99%)
25Mg amu (10.00%)
26Mg amu (11.01%)
What is the atomic mass of magnesium on the periodic table?
A) amu.
B) amu
C) amu

17. 40
20Ca2+ has
A) 20 protons, 20 neutrons, and 18
electrons.
B) 22 protons, 20 neutrons, and 20
C) 20 protons, 22 neutrons, and 18
D) 22 protons, 18 neutrons, and 18
E) 20 protons, 20 neutrons, and 22

18. 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
C) the name of the atom.
D) two of the above.
E) none of the above

19. If an atom of polonium (atomic number 84) undergoes a conversion to lead (atomic number 82) by the loss of a single particle,
A  the particle lost was an alpha particle 
 B  the particle lost was a gamma ray     
 C  the particle lost was a beta particle         
D  the particle lost could have been an
alpha particle or a beta particle
E  the particle lost was a positron

20. 0.98 g Li is equal to how many moles of Li and how many atoms of Li?
A  8.6 mol; 6.0 x 1023 atoms 
 B  0.14 mol; 8.6 x 1022 atoms     
 C  0.14 mol; 6.0 x 1023 atoms     
D  8.6 mol; 8.6 x 1022 atoms
E  you can’t tell both quantities

21. Z A z AX e-/m ratio John Dalton J. J. Thomson ions The Atom History
Chapter 3... HChem.
The Atom
counting them
Use D.A.
The MOLE
Hard Little Spheres
1 mole = 6.02 x 1023 = molar mass
History
John Dalton
Ernest Rutherford
J. J. Thomson
Planetary Model
Proust
Laviosier
Law of Definite ______
Gold Foil Exp.
Law of ______
Cathode Ray Tube Exp.
Democritus
Conservation
Compostion
The electron
(negatively charged matter)
Plum Pudding
Atom is mostly…
Nucleus (positive, dense core)
empty
model
Atomic Theory
These can be lost or gained
Atoms are indivisible
Nucleons
ions
1.76x108 C/g
1.6x10-19 C
Chadwick
Atoms rearrange in chem rxtions
e-/m ratio
All matter is comprised of atoms
Charge on the electron ________ Oil-Drop Exp.
Atoms of different elements have different masses
protons
neutrons
Millikan’s
(+ charge)
(no charge)
Atomic #
Mass #
Ionizing radiation
matter
mass of e- Z A
Element-A
9.11x10-28 g
nuclide
Alpha
A particular atom AX
Mass Spec.
Gamma
(Energy)
Beta
A group of z
Atomic masses
Equations to describe these
isotopes
Weighted Averages
radioactive
Most are…

22. A physical and endothermic
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  physical and endothermic 
 B  physical and exothermic     
 C  chemical and endothermic     
D  chemical and exothermic

23. A 576 °C 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.
2.) The temperature that Gallium melts is 303 K. That temperature on the centigrade scale is
A  576 °C 
 B  303 °C     
 C  100. °C     
D  30. °C
E 0.0 °C

24. A 59.1 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.
3.) If Michele poured the liquid gallium into a graduated cylinder what volume should she have found?
A  59.1 mL 
 B  0.591 mL     
 C  1.69 mL     
D  0.0591mL
E mL

25. A 13% 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  13%
 B  1.6 %     
 C  4.2 %     
D  0.69 %
E 6.5 %

26. Which of the following frequencies corresponds to light with the longest wavelength?
A) 3.00 x 1013 s–1
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

27. What is the energy of a photon of blue light that has a wavelength of 450 nm?
A) 6.7 x 1014 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

28. Define the term atomic orbital as best you can…..
High probability region in space where you’re likely to find an electron!

29. How many d orbitals have n = 3?
C) 10
D) 7
E) 18

30. How many electrons can be in the 1s orbital? ____ 2s? ____ 6s? ___
How many electrons can be in the 2p orbitals? ____ 3d? ____ 3f ? ___ 6 10
What is the shape of the s orbital? ________ 6s? ________
spherical
spherical
What is the shape of the p orbital? ________ 3d? ________
Clover (mostly)
dumbbell

31. Write the electron configuration notation for the element Indium
1s22s22p63s23p64s23d104p65s24d105p1

32. Which of these elements has three electrons in degenerate orbitals
Which of these elements has three electrons in degenerate orbitals?            A  Po          B  P          C  Hg          D  Si          E  Pd

33. Wave-like Particle-like l x n = c E = h n Wave Mechanical Model
Chapter 4 H Chem
The Rutherford Model could not explain…
The Atom…cont’d
The atom does not collapse
The light emitted by atoms
(Photo-electric effect)
For hydrogen:
(Young…Double Slit)
(Planck / Einstein)
Bright-Line Spectra
Wave-like
Particle-like
3.0 x 108m/s
(What atoms have to do with it)
l x n = c
E = h n
-1312 kJ
wavelength
For H:
En=
mole e- n2
frequency
Speed of light
Quantum of energy
(photon)
Bohr Model
Wave Mechanical Model
Planck’s Constant… 6.6x10-34J•s
electrons can have only certain energies
colors are emitted when electrons jump from higher to lower energy levels
The observer affects the observed
What DeBroglie said
Therefore
Energy levels exist
Heisenberg’s Uncertainty Principle
If light has a dual nature…why not matter
Schroedinger
(Proven by looking at Bright-Line Spectra)
(Max Born)
Sub-levels exist
Electrons are waves of chance.
Electrons are standing waves…only certain energies allowed
These are called:
Defined as:
orbitals
Shown with: 1. or 2. s
(1) p
(3) d
(5) f
(7)
Aufbau
High probability regions in space where the electron is likely to be found
Config.
Pauli
Filling order for atoms with more than one electron
Hund’s
Orbital

34. 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

35. An element having the configuration [Xe]6s1 belongs to the Group:     A  halogens 
    B  None of these        
  C  alkaline earth metals 
D  alkali metals
    E  noble gases

36. 1. Is phosphorous a metal or non- metal?
2.Write the orbital notation for the
element phosphorous.
3. What is the charge on the
phosphide ion?
4. How many neutrons are in a
phosphorous atom?
5. Which is bigger, the atom or the ion?
nonmetal
1s22s22p63s23p3 3-
You can’t tell…
the ion!

37. Of the following elements, which has the lowest first ionization energy?
A) Ba
B) Ca
C) Si
D) P
E) Cl

38. ←Trends The Periodic Table Terms Dobereiner Based on Mass Families
Chapter 5 -- H. Chemistry
The Periodic Table
(repetition of behavior)
Terms
Dobereiner
know the “groups”
Based on Mass
Families
Triads
Periods
Newlands
Metals/Nonmetals
Octaves
“father” of the periodic chart
Metalloids
Mendeleev
←Trends
Blocks
left blanks
First Chart
Isoelectronic
Moseley
Valence**
Based on atomic number
Periodic Law
**outermost s and p electrons
Metallic Reactivity
Reasons (based on structure)
Metallic Character
Atomic Size
Nuclear Charge
know the transition to these
Ionic Size
across
Higher Energy Levels
down
Charge
Ionization Energy
Electron Affinity

39. 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 test is used to determine if a sample of gas is CO2?

40. What is the hybridization on each oxygen atom in a molecule of oxygen?
A) sp
B) sp2
C) sp3
D) dsp3
E) d2sp3

41. Which of the following molecules has a dipole moment. (i. e
Which of the following molecules has a dipole moment? (i.e. is a polar molecule)
A) BCl3
B) SiCl4
C) PCl3
D) Cl2
E) none of these

42. Exceptions to octet rule
General Properties
Chapter 6 Honors Chem.
General Properties
Soluble in water
Insoluble in water
Conductive in sol’n
Chemical Bonding
Nonconductive in sol’n
Higher M.P.’s
Lower M.P.’s
IONIC...transfer
Lowers energy of system
Rationale:
COVALENT...sharing
Accompanied by:
Accompanied by:
Process (steps)
I.E
A Blend
E.A
How to tell
Pauling
L.E.
Polar Covalent… unequal sharing
Person Responsible
Electro- negativity
>1.7
0.0 – 0.3
differences
2-D Lewis Structures
Resonance
^and 3-D**
Guidelines
Count
d- d+
Connect
Exceptions to octet rule
Multiple Bonds
Polarity of bonds
Distribute

43. Multiple bonds count the same as single bonds
Honors Chem.
Molecular Shapes
dictated by
nonpolar
polar
(symmetrical)
(nonsymmetrical)
Polarity of Molecules V S E P R
Theory
shows
(when atom arrangements vary)
alence
air
isomerism
hell
**3-D Lewis Structures
lectron
epulsion
from this you
resonance
CH4
(when one bonding arrangement is insufficient)
NH3
H2O
can create
BF3
109.5° angles
107° angles
104.5° angle
120° angles
Example # of bonds** # of lone pairs EPA Shape Hybridization
CH4 4
SO2
tetrahedral
tet.
sp3
NH3 3 1
tet.
trig. pyramidal
sp3
H2O 2 2
tet.
bent
sp3
<120° angle
possible scenarios
BF3 3
trig. planar
trig. planar
sp2
SO2 2 1
trig. planar
bent
sp2
CO2 2
linear
linear sp
180° angle
Multiple bonds count the same as single bonds **