Which set of quantum numbers cannot occur together to specify an orbital?
a. n=4,l=3,ml=3
b. n=2,l=1,ml=?1
c. n=3,l=2,ml=3
d. n=3,l=2,ml=0
C
How many orbitals are present when l=3?
1
3
5
7
9
7
How many 8p orbitals exist?
ANSWER:
3
1
0
8
5
3
Each set of quantum numbers is supposed to specify an orbital. However, each set contains one quantum number that is not allowed. Replace the quantum number that is not allowed with one that is allowed.
n=3;l=3;ml=+2
a. ml=0
b. n=4
c. l=4
d. n=2
b
The number of 2s electrons in Be.
2
The number of 3d electrons in Co.
7
The number of 4p electrons in As.
3
The number of 3d electrons in V.
3
Write the correct electron configuration for S.
Express your answer in complete form,
1s^22s^22p^63s^23p^4
The element that corresponds to the electron configuration 1s^22s^22p^63s^23p^64s^13d^5 is ________.
a. vanadium
b. chromium
c. titanium
d. manganese
e. iron
b
Which of the following statements is TRUE?
ANSWER:
a. An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
b. Two electrons in
c
Why does an electron found in a 2s orbital have a lower energy than an electron found in a 2p orbital in multielectron systems?
ANSWER:
a. There are more nodes found in the 2s orbital.
b. Electrons in the 2s orbital are shielded by electrons in the 2p.
c.
e
Give the ground state electron configuration for I.
ANSWER:
a. [Kr]5s^24d^105p^5
b. [Kr]5s^25p^6
c. [Kr]4d^105p^6
d. [Kr]5s^25d^105p^6
e. [Kr]5s^24d^105p^6
a
Use the periodic table to determine the electron configuration of bismuth (Bi).
Express your answer in condensed form.
[Xe]4f^145d^106s^26p^3
Use the periodic table to determine the electron configuration for iodine (I).
Express your answer in condensed form.
[Kr]5s^24d^105p^5
The shell number is equal to the n value. The type of subshell corresponds to the ? value.
Type of
subshell ?
s..................0
p.................1
d................ 2
f..................3
If an element is located in the fourth column of the 7p block of the periodic table, which of the following would you expect to find in its electron configuration?
ANSWER:
a.4p^7
b.7p^4
c.s4p^7
d.p^11
b
[Kr]5s24d105p2
Express your answer as a chemical symbol.
ANSWER:
Sn
The number of 3s electrons in Na.
Express your answer as an integer.
ANSWER:
1
The number of 3d electrons in Cr.
Express your answer as an integer.
ANSWER:
5
Choose the statement that is TRUE.
ANSWER:
a. Core electrons are the easiest of all electrons to remove.
b. Outer electrons efficiently shield one another from nuclear charge.
c. Valence electrons are most difficult of all electrons to remove.
d. Core ele
d
Determine the number of valence electrons for each of the following four elements.
Ga
Express your answer as an integer.
ANSWER:
3
Elements with 3 or fewer valence electrons tend to lose electrons, and elements with 5 or more valence electrons tend to gain electrons.
Thus, Ga and Pb tend to lose electrons, whereas Cl and Se tend to gain electrons.
According to Hund's rule, the electrons will arrange in the degenerate set of orbitals with one electron in each orbital with like spins before any pairing occurs. So for Hund's violation to occur the subshell must have a degenerate set of orbitals.
In wh
d
In an orbital diagram, the arrows are used to indicate the relative spin of an electron (indicative of its ms value). Which of the following correctly describes a violation of the Pauli exclusion principle?
ANSWER:
a. Arrows in the same orbital with the s
a
How is the electron configuration of an anion different from that of the corresponding neutral atom?
ANSWER:
a. add the number of electrons required by the magnitude of the charge of the anion
b. subtract the number of electrons required by the magnitude
a
How is the electron configuration of a cation different?
ANSWER:
a. add the number of electrons required by the magnitude of the charge of the cation
b. subtract the number of electrons required by the magnitude of the charge of the cation
c. the electron
b
Group Tendency Charge
1A... Lose one electron... +1
2A... Lose two electrons +2
3A Lose three electrons +3
5A Gain three electrons -3
6A Gain two electrons -2
7A Gain one electron -1
8A Rarely gain or lose electrons 0
yep
Identify the preceding noble gas for a metal
Beryllium, Be, is located in group 2A and in period 2 of the periodic table. Identify the preceding noble gas.
ANSWER:
a.helium
b.neon
c.argon
Identify the succeeding noble gas for a nonmetal
Bromine, Br, is lo
a
b
As
Express your answer as an ion.
Rb
Express your answer as an ion.
ANSWER:
As3?
ANSWER:
Rb+
Rank from largest atomic radius to smallest
Ca
Mg
Be
Sr
Sr Ca Mg Be
How many protons and how many inner (nonvalence) electrons does a neutral boron atom have?
Express your answers as integers separated by a comma.
ANSWER:
5, 2
How many protons and how many inner (nonvalence) electrons does a neutral oxygen atom have?
Express your answers as integers separated by a comma.
ANSWER:
8, 2
On the basis of periodic trends, choose the larger atom in each pair (if possible).
Part A
Al or S
a.Al
b.S
c. It is impossible to determine based on periodic trends alone.
Part B
Ge or Po
ANSWER:
a.Ge
b.Po
c.It is impossible to determine based on periodi
a
c
b
b
Arrange the following atoms according to decreasing effective nuclear charge experienced by their valence electrons: S, Na, Al, and Si.
Largest) S Si Al NA (Smallest
Write the electron configuration for Zn2+?
Express your answer in condensed form
ANSWER:
[Ar]3d^10
Write the electron configuration for V3+
[Ar] 3d^2
Write the electron configuration for Mo3+
[Kr]4d^3
of
1s^22s^22p^63s^23p^64s^23d^104p^65s^04d^3.
Write the electron configuration for O2?
[He]2s^22p^6
Enter the condensed electron configuration for the following three ions:
Co2+
N3?
Ca2+
Express your answers in condensed form separated by commas.
[Ar]3d^7, [He]2s^22p^6, [Ar]
On the basis of periodic trends, determine the element in each pair with the higher first ionization energy (if possible).
Sn or I
ANSWER:
a.Sn
b.I
c.It is impossible to determine based on periodic trends alone.
Part B
Ca or Sr
ANSWER:
a.Ca
b.Sr
c.It is i
B
A
C
A
Arrange the following elements in order of decreasing first ionization energy: Po, Cl, Te, and Se.
Laregest) Cl Se Te Po (smallest
Choose the element with the highest first ionization energy from each of the following pairs.
Part A
Kr or Br
ANSWER:
a. Kr
b. Br
Part B
Na or Rb
ANSWER:
a. Na
b. Rb
Part C
Rn or Pb
ANSWER:
a. Rn
b. Pb
Part D
S or Sb
ANSWER:
a. S
b. Sb
all A
identify the energy change that occurs when an electron is added to a neutral gaseous O atom, forming an O? ion:
O(g)+e??O?(g)
ANSWER:
a. ?710 kJ
b. +142 kJ
c. ?142 kJ
d. +710 kJ
c
identify the energy change that occurs when an electron is added to an O? ion, forming an oxide (O2?) ion:
O?(g)+e??O2?(g)
ANSWER:
a. ?142 kJ
b. +710 kJ
c. +142 kJ
d. ?710 kJ
b
For the elements with the electron affinities given in the table in the introduction, which element is most likely to accept an electron?
Hint 1. How to interpret electron affinity values
The values of electron affinity are given in kilojoules per mole. N
a
On the basis of periodic trends, choose the more metallic element from each pair (if possible).
Part A
Ge or Sn
ANSWER:
a. Ge
b. Sn
c. It is impossible to determine based on periodic trends alone.
Part B
Sb or Po
ANSWER:
a. Sb
b. Po
c. It is impossible to
B
C
B
A
What type of bonding occurs in iron(III) chloride, FeCl3?
covalent
metallic
ionic
ionic
What type of bonding occurs in a sample of pure copper, Cu? In other words, how is one copper atom held to another copper atom?
covalent
metallic
ionic
metallic
Determine the empirical formula for the compound represented by each molecular formula.
Part A
N2O4
Express your answer as a chemical formula.
Part B
C5H12
Express your answer as a chemical formula.
Part C
C4H10
Express your answer as a chemical formula.
ANSWER:NO2..... (small subscripts)
ANSWER:C5H12..... (small subscripts)
ANSWER:C2H5..... (small subscripts)
identify the nobel gas proceeding the metal
Li, lithium, is located in group 1A and in period 2 of the periodic table. Identify the preceding noble gas.
ANSWER:
a.helium
b.neon
c.argon
Hint 4. Identify the noble gas succeeding a nonmetal
Se, selenium, is
A
B
Determine the number of valence electrons in the neutral nonmetals
How many valence electrons are in a neutral atom of As, Se, and Br, respectively?
Express your answer as three integers separated by commas.
Hint 2. Determine the number of valence electro
ANSWER:
5,6,7
ANSWER:
1,2,3
Hint 1. Balance the charges in an example compound
How many Y2? anions are needed to balance the charge on one X+6 cation?
Express your answer numerically as an integer.
ANSWER:
3
Write a formula for the ionic compound that forms between each pair of elements.
Part A
magnesium and chlorine
Express your answer as a chemical formula.
Part B
barium and oxygen
Express your answer as a chemical formula.
Part C
strontium and sulfur
Expre
ANSWER:
MgCl2..... (small subscripts)
ANSWER:
BaO..... (small subscripts)
ANSWER:
SrS..... (small subscripts)
ANSWER:
BeCl2..... (small subscripts)
Write a formula for the compound that forms between calcium and each polyatomic ion:
Part A
hydroxide
Express your answer as a chemical formula.
Part B
chromate
Express your answer as a chemical formula.
Part C
phosphate
Express your answer as a chemical
ANSWER:
Ca(OH)2..... (small subscripts)
ANSWER:
CaCrO4..... (small subscripts)
ANSWER:
Ca3(PO4)2..... (small subscripts)
ANSWER:
Ca(CN)2..... (small subscripts)
Name each ionic compound.
Part A
Mg3P2
Spell out the full name of the compound.
Part B
KBr
Spell out the full name of the compound.
Part C
NaBr
Spell out the full name of the compound.
Part D
Li2S
Spell out the full name of the compound.
Part E
CsF
Spell
ANSWER:
magnesium phosphide
ANSWER:
potassium bromide
ANSWER:
sodium bromide
ANSWER:
lithium sulfide
ANSWER:
cesium fluoride
ANSWER:
potassium iodide
Name each ionic compound.
Part A
SnBr4
Spell out the full name of the compound.
Part B
PbF4
Spell out the full name of the compound.
Part C
FeO
Spell out the full name of the compound.
Part D
CuO
Spell out the full name of the compound.
Part E
FeCl2
Spell
ANSWER:
tin(IV) bromide
ANSWER:
lead(IV) fluoride
ANSWER:
iron(II) oxide
ANSWER:
copper(II) oxide
ANSWER:
iron(II) chloride
ANSWER:
nickel(II) chloride
Give each ionic compound an appropriate name.
Part A
SnI4
Spell out the full name of the compound.
Part B
CrS
Spell out the full name of the compound.
Part C
RbI
Spell out the full name of the compound.
Part D
BaBr2
Spell out the full name of the compound
ANSWER:
tin(IV) iodide
ANSWER:
chromium(II) sulfide
ANSWER:
rubidium iodide
ANSWER:
barium bromide
Give the systematic name for the compound Fe2(SO4)3.
iron(III) sulphate
Give the systematic name for the compound NaNO3.
nitrate
Enter the formula for the compound barium oxide.
BaO
Enter the formula for the compound lead(II) phosphate.
Pb3(PO4)2..... (small subscripts)
Prefix Number
mono.....one
di............two
tri...........three
tetra.......four
penta.......five
hexa........six
hepta........seven
octa ...........eight
nona.......nine
deca.......... ten
yep
What is the name for the compound CCl4?
What is the name for the compound P4O10
carbon tetrachloride
tetraphosphorus decoxide
What is the formula for the compound nitrogen monoxid
What is the formula for the compound methane?
NO
CH4..... (small subscripts)
Name each of the following molecular compounds.
Part A
SO3..... (small subscripts)
Spell out the full name of the compound.
Part B
SO2..... (small subscripts)
Spell out the full name of the compound.
Part C
RnF2..... (small subscripts)
Spell out the full
ANSWER:
sulfur trioxide
Correct
ANSWER:
sulfur dioxide
ANSWER:
radon difluoride
ANSWER:
nitric oxide
Calculate the formula mass for each of the following compounds.
Part A
AgCl
Express your answer using two decimal places.
Part B
PBr3..... (small subscripts)
Express your answer using two decimal places.
Part C
CH3CONH2..... (small subscripts)
Express you
ANSWER:
formula mass = 143.32 amu
ANSWER:
formula mass = 270.67 amu
ANSWER:
formula mass = 59.07 amu
ANSWER:
formula mass = 163.94 amu
Find the number of ibuprofen molecules in a tablet containing 200.0 mg of ibuprofen (C13H18O2).
Express the amount to four significant figures.
Part B
What is the mass of a sample of water containing 3.55�1022 molecules of H2O?
Express the mass in grams t
ANSWER:
amount = 5.839�1020 molecules of C13H18O2
ANSWER:
mass = 1.06 g
Determine the mass of oxygen in a 7.2-g sample of Al2(SO4)3.
Express the mass in grams to two significant figures.
Part B
Butane (C4H10) is the liquid fuel in lighters. How many grams of carbon are present within a lighter containing 7.25 mL of butane? (T
ANSWER:
mass of oxygen = 4.0g
ANSWER:
mass of carbon = 3.60g
Acetic acid (C2H4O2) is the active ingredient in vinegar.
Part A
Calculate the mass percent composition of oxygen in acetic acid.
Express your answer using four significant figures.
..... (small subscripts)
ANSWER:
Mass % = 53.29%
Copper (II) fluoride contains 37.42% F by mass.
Part A
Use this percentage to calculate the mass of fluorine (in g) contained in 59.5 g of copper (II) fluoride.
ANSWER:
mF = 22.3g
Silver chloride, often used in silver plating, contains 75.27% Ag.
Part A
Calculate the mass of silver chloride required to plate 225 mg of pure silver.
ANSWER:
mAgCl = 299mg
A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume you have a 100.-g sample of this compound.
Part A
How many grams of each element are in this sample?
Enter the number of grams of carbon followed by the number of grams of hydrogen, separated b
ANSWER:
mass of C, mass of H = 80.0,20.0g
ANSWER:
moles of C, moles of H = 6.66,19.8mol
ANSWER: CH3 ..... (small subscripts)
ANSWER: C2H6..... (small subscripts)
The empirical formula and molar mass of several compounds are listed below. Find the molecular formula of each compound.
Part A
C6H7N, 186.28 g/mol
Express your answer as a chemical formula.
Part B
C2HCl, 120.95 g/mol
Express your answer as a chemical for
ANSWER: C12H14N2..... (small subscripts)
ANSWER:C4H2Cl2..... (small subscripts)
ANSWER:
C20H40N4S8..... (small subscripts)
In the molecule FCl, which atom is the negative pole?
F
Of the molecules HF and HCl, which has bonds that are more polar?
HF
Both of the sulfur-chlorine single bonds in SCl2..... (small subscripts) are polar. In which direction should the polarity arrows point?
ANSWER:
a. to the right
b. to the left
c. toward the central sulfur atom
d. away from the central sulfur atom
hint: Th
D
Part A
Determine if the bond formed between I and I is pure covalent, polar covalent, or ionic.
ANSWER:
a. polar covalent
b. ionic
c. pure covalent
Part B
Determine if the bond formed between Cs and Br is pure covalent, polar covalent, or ionic.
ANSWER:
a
c
a
c