G10 Advanced Chemistry
Chapter 1 Revision Sheet-Answer Key
Multiple Choice Questions.
Q1.
Cosmic rays are high-energy radiation from outer space. What is the frequency of a cosmic ray
that has a wavelength of 2.67 × 10-13 m when it reaches Earth? (The speed of light is 3.00 × 108
m/s.)
a.
b.
c.
d.
8.90 × 10-22 s-1
3.75 × 1012 s-1
8.01 × 10-5 s-1
1.12 × 1021 s-1
Q2.
Which is the electron-dot structure for indium?
a.
b.
c.
d.
Q3.
a.
b.
c.
d.
To which sublevel do all of these orbitals belong?
s
p
d
f
1
Q4.
How many electrons total can reside in this sublevel?
a.
b.
c.
d.
2
3
6
8
Q5.
What is the maximum theoretical number of electrons related to the fifth principal energy level
of an atom?
a.
b.
c.
d.
2
8
18
32
Q6.
a.
Using noble-gas notation, what is the ground-state electron configuration of Cd?
[Kr]4d104f2
b.
[Ar]4s23d10
c.
[Kr]5s24d10
d.
[Xe]5s24d10
Q7.
What is the element that has the ground-state electron configuration [Xe]6s24f145d6?
a.
b.
c.
d.
La
Ti
W
Os
2
Q8.
What is the complete electron configuration of a scandium atom?
a.
1s22s22p63s23p64s23d1
b.
1s22s22p73s23p74s23d1
c.
1s22s22p53s23p54s23d1
d.
1s22s12p73s13p74s23d1
Q9.
Which is NOT evidence that a chemical change has occurred?
a.
b.
c.
d.
The properties of the substances involved in the reaction have changed.
An odor is produced.
The composition of the substances involved in the reaction have changed.
The total mass of all substances involved has changed.
Use the diagram below to answer Q10 and Q11.
Q10. Which shows an orbital diagram that violates the Aufbau principle?
a.
b.
c.
d.
A
B
C
D
Q11. In the diagram in Q10 Which one shows the orbital diagram for the element beryllium?
a.
b.
c.
d.
A
B
C
D
3
Q12. A student performs an experiment to measure the boiling point of pentane and measures it at
37.2°C. The literature reports this value as 36.1°C. What is the student’s percent error?
a.
b.
c.
d.
97.0%
2.95%
1.1%
3.05%
Q13. Which method of separating components of a mixture depends on the different boiling points of
the components of the mixture?
a.
b.
c.
d.
chromatography
filtration
crystallization
distillation
Q14. Germanium is an element in periodic table with the symbol Ge and an atomic number of 32.
What is the correct electron configuration of Germanium?
a.
b.
c.
d.
[Ar]3d94s34p²
[Ar]3d¹⁰4s²4p2
[Ar]3d¹⁰4s14p3
[Ar]3d94s²4p3
Q15. 1s22s22p63s23p64s23d6 is the electron configuration of which element in the periodic table?
a.
b.
c.
d.
Manganese, Mn
Nickel, Ni
Cobalt, Co
Iron, Fe
4
Constructed Response Questions.
Q1
a.
Define the following terms.
a. frequency b. wavelength
c. quantum d. ground state
a. Frequency is the number of waves that pass a given point per second.
b. Wavelength is the shortest distance between equivalent points on a continuous wave.
c. A quantum is the minimum amount of energy that can be lost or gained by an atom.
d. An atom’s ground state is its lowest allowable energy state
b.
Arrange the following types of electromagnetic radiation in order of increasing wavelength.
a. ultraviolet light b. microwaves c. radio waves d. X-rays
d. X-rays,
a. ultraviolet light,
b. microwaves,
c. radio wave
c.
What is the photoelectric effect?
Photoelectric effect is a phenomenon in which a metal emits electrons when light of a sufficient
frequency shines on it.
5
Q2
a.
What is an atomic orbital and what does n represent in the quantum mechanical model of the
atom?
An atomic orbital is a three-dimensional region around the nucleus describing an electron’s
probable location
n represents an orbital’s principal quantum number, which indicates the relative size and
energy of the orbital.
b.
In what sequence do electrons fill the atomic orbitals related to a sublevel?
Each orbital must contain a single electron before any orbital contains two electrons.
6
c.
What element is represented by each electron configuration?
a. [Ar]4s2
b. [Xe]6s24f4
c. [Kr]5s24d105p4
d. [Rn]7s25f13
f. 1s22s22p63s23p64s23d104p5
a. F
b. Ca
c. Nd
d. Te
e. Md
f. Br
7
G10 Advanced Chemistry
Chapter 2 - Revision Sheet - Answer Key
Multiple Choice Questions.
Q1.
Identify which of the following is a metal?
a.
b.
c.
d.
Germanium
Oxygen
Iron
Fluorine
Q2.
Identify which of the following is a nonmetal?
a.
Silicon
b.
c.
Chlorine
Sodium
d.
Carbon
Q3.
Identify which of the following is a metalloid?
a.
b.
c.
d.
Mercury
Argon
Calcium
Tellurium
Q4.
Identify the corresponding group number of noble gases in the periodic table?
a.
b.
c.
d.
Group 1
Group 2
Group 17
Group 18
1
Q5.
Identify the corresponding group number of alkali metals in the periodic table?
a.
b.
c.
d.
Group 1
Group 2
Group 17
Group 18
Q6.
Elements in the same group of the periodic table have the same --------------------------?
a.
b.
Number of valence electrons
Physical properties.
c.
d.
Number of electrons
Electron configuration
Q7.
Which statement is NOT true?
a.
b.
c.
d.
The atomic radius of Na is less than the atomic radius of Mg.
The electronegativity of C is greater than the electronegativity of B.
The ionic radius of Br − is greater than the atomic radius of Br.
The first ionization energy of K is greater than the first ionization energy of Rb.
Q8.
a.
What is the group, period, and block of an atom with the electron configuration
[Ar]4s23d104p4?
group 14, period 4, d-block
b.
c.
group 16, period 3, p-block
group 14, period 4, p-block
d.
group 16, period 4, p-block
2
Use the table below to answer Q9 and Q10
Q9.
In which group does Element X most likely belong?
a.
1
b.
c.
17
18
d.
4
Q10. Using the table in Q9 above, find out in which block is Element Z most likely found?
a.
b.
c.
d.
s-block
p-block
d-block
f-block
Use the table below to answer Questions 11 and 12
Q11. What is the percent nitrogen in the compound N O ?
2 3
a.
b.
c.
d.
44.7%
46.7%
28.1%
36.8%
3
Q12. A sample of a nitrogen oxide contains 1.29 g of nitrogen and 3.71 g of oxygen. Using the table in
Q11 find out which compound is this most likely to be?
a.
N 2O 4
b.
N 2O 3
c.
N 2O
d.
N 2O 5
Q13. On the modern periodic table, metalloids are found only in
a.
b.
c.
d.
the d-block.
groups 13 through 17.
the f-block.
groups 1 and 2
Q14. Which group is composed entirely of nonmetals?
a.
b.
c.
d.
1
13
15
18
Q15. It can be predicted that element 118 would have properties similar to a(n)
a.
b.
c.
d.
alkali earth metal.
halogen.
metalloid.
noble gas.
4
Constructed Response Questions.
Q1
a.
Write the electron configuration for the element arsenic (As).
1s22s22p63s23p64s23d104p3
Use the table below to answer parts b and c.
b.
Correlate the biggest jump in ionization energy to the number of valence electrons in each atom.
It is easier to remove valence electrons from a partially filled shell. For lithium, it requires much
more energy to remove the second electron than the first because the second electron is part of a
completely filled outer shell. Its removal causes the atom to become unstable, and therefore
requires a great deal of energy to remove.
Similarly, for beryllium, it requires much more energy to remove the 3 rd electron, for boron, it
requires much more energy to remove the 4 th electron and for carbon, it requires much more
energy to remove the 5 th electron as all these removals cause the atoms to become unstable and
requires a great deal of energy to remove.
c.
Predict which ionization energy will show the largest jump for magnesium. Explain your
answer.
Magnesium will have its largest increase in ionization energy for the third ionization energy.
The first two ionization energies are how much energy it requires to remove magnesium’s two
valence electrons. The third ionization energy will disrupt a complete octet, and therefore
requires a lot more energy.
5
Q2
a.
Determine the group, period, and block in which each of the following elements is located in the
periodic table.
a. [Kr]5s24d1 b. [Ar]4s23d104p3 c. [He]2s22p6 d. [Ne]3s23p1
a.
b.
c.
d.
b.
3, period 5, d-block
15, period 4, p-block
18, period 2, p-block
13, period 3, p-block
Given any two elements within a group, is the element with the larger atomic number likely to
have a larger or smaller atomic radius than the other element?
Larger
c.
Table below shows the number of elements in the first five periods of the periodic table. Explain
why some of the periods have different numbers of elements?
The first energy level has only the s sublevel. The second and third energy levels have only the s
and p sublevels. The fourth and fifth energy levels have s, p, and d sublevels.
6
G10 Advanced Chemistry
Chapter 3 Revision Sheet - Answer Key
Multiple Choice Questions.
Q1.
Which of the following atom has two valence electrons in its outer most shell?
a.
b.
c.
d.
cesium
rubidium
gallium
zinc
Q2.
Arrange the following atoms in the order of highest reactivity to the lowest reactivity based on
their electron configuration.
a.
chlorine fluorine neon bromine
b.
fluorine neon bromine chlorine
c.
d.
Neon chlorine bromine fluorine
Fluorine chlorine bromine neon
Q3.
Which description is supported by the model shown above?
a.
b.
c.
d.
Metals are shiny, reflective substances.
Metals are excellent conductors of heat and electricity.
Ionic compounds are malleable compounds.
Ionic compounds are good conductors of electricity.
Q4.
Which is NOT true of the Sc 3+ ion?
a.
b.
c.
d.
It has the same electron configuration as Ar.
It is a scandium ion with three positive charges.
It is considered to be a different element than a neutral Sc atom.
It was formed by the loss of 4s and 3d electrons.
1
Q5.
Of the salts below, which would require the most energy to break an ionic bond?
a.
b.
c.
d.
BaCl2
Li F
Na Br
K
Q6.
The high strength of its ionic bonds results in all of the following properties of NaCl except
a.
hard crystals.
b.
high boiling point.
c.
high melting point.
d.
low solubility
Q7.
Which is the correct formula for the compound chromium (III) sulfate?
a.
b.
c.
d.
Cr3SO4
Cr2(SO4)3
Cr3(SO4)2
Cr(SO4)3
Use the table below to answer questions 8 to 10
2
Q8.
A compound is discovered to have a melting point of -100°C. Which could be true of this
compound?
a.
It definitely has an ionic bond.
b.
It definitely has a polar covalent bond.
c.
It has either a polar covalent bond or a nonpolar covalent bond.
d.
It has either a polar covalent bond or an ionic bond
Q9.
In the table above Q8 which could NOT be the melting point of Cr 2O3?
a.
2375°C
b.
c.
950°C
148°C
d.
3342°C
Q10. In the table above Q8 which is supported by the data in the table?
a.
b.
c.
d.
Nonpolar covalent bonds have high boiling points.
Polar covalent bonds have high melting points.
Ionic bonds have low melting points.
Ionic bonds have high boiling points.
Q11. How many valence electrons does Rubidium Rb has in its outer most shell?
a.
b.
c.
d.
3
4
1
2
Use the following figure to answer questions 12 to 15
3
Q12. Which element in the above figure has 7 valence electrons and what ion will it form?
a.
b.
c.
d.
B and Ba +2
C and Rb+1
F and No ion will form
E and I-1
Q13. In the figure above Q12 which element will donate one electron to element E to make an ionic
compound with F?
a.
b.
c.
d.
E
C
B
A
Q14. In the figure above Q12 which element will donate two electrons to element E to make an ionic
compound with?
a.
E
b.
C
c.
B
d.
A
Q15. In the figure above Q12 how many electrons does element A has in its outer most shell and
which ion will it form?
a.
3 and Al+3
b.
2 and A+2
c.
5 and N-3
d.
6 and Se-2
4
Constructed Response Questions.
Q1
a.
Give the number of valence electrons for each atom in the following elements.
a. cesium b. rubidium c. gallium d. zinc e. strontium
Ans
a. 1
b. 1
c. 3
d. 2
e. 2
b.
Determine the ratio of cations to anions in each of the following.
a. potassium chloride, a salt substitute
b. calcium fluoride, used in the steel industry
c. calcium oxide, used to remove sulfur dioxide from power-plant exhaust
d. strontium chloride, used in fireworks
Ans
a. 1:1 b. 1:2 c. 1:1 d. 1:2
c.
Complete table 14 by placing the symbols, formulas, and names in the blanks.
Ans
NH4+; SO42-; ammonium sulfate; (NH 4)2SO4
Pb2+; F-; lead (II) fluoride; PbF2
Li+; Br-; lithium bromide; LiBr
Na +; CO32- ; sodium carbonate; Na 2CO3
Mg 2+; PO43- ; magnesium phosphate; Mg 3(PO4)2
5
Q2
a.
Give the formula for each ionic compound.
a. calcium iodide
b. silver bromide
c. copper (II) chloride
d. potassium periodate
e. silver acetate
Ans
a. CaI2 b. AgBr
c. CuCl2
d. KIO 4
e. AgC2H3O2
b.
Name each of the following ionic compounds.
a. K2O b. CaCl2 c. Mg 3N2 d. NaClO e. KNO3
Ans
a.
b.
c.
d.
e.
c.
Briefly explain why steel, an alloy of iron, is used to build the supporting structure of many
buildings?
Ans
Iron forms a strong metallic bond, giving solid iron hardness and strength.
potassium oxide
calcium chloride
magnesium nitride
sodium hypochlorite
potassium nitrate
6
G10 Advanced Chemistry
Chapter 4 - Revision Sheet – Answer Key
Multiple Choice Questions.
Q1.
Covalent bonds form when atoms ____________ one or more pairs of electrons
a.
b.
c.
d.
donate
accept
share
shrink
Q2.
Bond length is measured ________________ to nucleus.
a.
b.
outer most electron
Inner most electron
c.
d.
proton
nucleus
Q3.
Molecules that produce _________ in solution are acids.
a.
b.
c.
d.
H+ ions
H- ions
OH- ions
OH+ ions
Q4.
_____________ bonds occur when electrons are not shared equally forming a dipole.
a.
b.
c.
d.
Non-polar
polar
ionic
Triple
Q5.
The __________________ difference determines the character of a bond between atoms.
a.
b.
c.
d.
electron affinity
bond length
atomic radius
electronegativity
1
Q6.
The common name of SiI 4 is tetraiodosilane. What is its IUPAC molecular compound name?
a.
b.
c.
d.
silane tetraiodide
silane tetraiodine
silicon iodide
silicon tetraiodide
Q7.
Which compound contains at least one pi bond?
a.
b.
c
d.
CO2
CHCl3
AsI3
BeF2
Q8.
Use the graph below to answer Q8 and Q9
What is the electronegativity of the element with atomic number 14?
a.
1.5
b.
1.8
c.
2.6
d.
2.2
2
Q9.
Referring to the graph in Q8, an ionic bond would form between which pairs of elements?
a.
b.
atomic number 3 and atomic number 4
atomic number 7 and atomic number 8
c.
d.
atomic number 4 and atomic number 18
atomic number 8 and atomic number 12
Q10. Which is the Lewis structure for silicon disulfide?
a.
b.
c.
d.
Q11. The central selenium atom in selenium hexafluoride forms an expanded octet. How many
electron pairs surround the central Se atom?
a.
b.
c.
d.
4
5
6
7
Q12. Use the table below to answer questions 12 and 13.
Which diatomic gas has the shortest bond between its two atoms?
a.
b.
c.
d.
HI
O2
Cl2
N2
3
Q13. Referring to the table in Q12, approximately how much energy will it take to break all the bonds
present in the molecule below?
a.
b.
c.
d.
3024 kJ/mol
4318 kJ/mol
4621 kJ/mol
5011 kJ/mol
Q14. Which compound does NOT have a bent molecular shape?
a.
b.
c.
d.
BeH2
H 2S
H 2O
SeH2
Q15. Which compound is nonpolar?
a.
b.
c.
d.
H 2S
CCl4
SiH3Cl
AsH3
4
Constructed Response Questions.
Q1
a.
What is the octet rule, and how is it used in covalent bonding?
Ans.
Atoms lose, gain, or share electrons to achieve an octet. Covalent bonding occurs when atoms
share electrons to achieve an octet.
b.
Give the number of valence electrons in N, As, Br, and Se. Predict the number of covalent bonds
needed for each of these elements to satisfy the octet rule?
Ans.
N: 5, 3; As: 5, 3; Br: 7, 1; Se: 6, 2
c.
Complete Table 8.
Ans.
HClO2: chlorous acid; H 3PO4: phosphoric acid; H 2Se: hydroselenic acid; HClO 3: chloric acid
5
Q2
a.
Draw the Lewis structures for these molecules, each of which has a central atom that does not
obey the octet rule.
a. PCl5
b. BF3
c. ClF5
d. BeH2
Ans.
a.
b.
What is the basis of the VSEPR model?
Ans.
The repulsive nature of electron pairs around a central atom
c.
Complete Table 9 by identifying the expected hybrid on the central atom. You might find
drawing the molecule’s Lewis structure helpful.
Ans.
b.
c.
XeF4: sp3d2; TeF4: sp3d; KrF2: sp3d; OF2: sp3
6
d.