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WorksheetsCHEM II
Total questions: 21
Worksheet time: 12mins
Which of the following compounds would contain ionic bonds?
BaCl2
LiNO3
NH3
CCl4
both a) and b)
Which of the following elements would form an ion with a charge of 3+ ?
nitrogen
phosphorus
aluminum
strontium
all of the above
How many groups of elements are found in the p-block of the periodic table?
2
4
6
10
14
Which of the following is the correct electron configuration for a Sb atom in the ground state?
[Kr]5s2 4d10 5p3
[Ar]4s2 5d10 5p3
[Kr]5s2 5d10 5p3
[Xe]5s2 5d10 5p3
[Kr]5d10 5p3
Which series contains ONLY atoms and ions with the same number of protons?
Cl-, Ar, Ca2+
O2-, N-, F-
Li+, Ba+, Rb+
Fe, Fe2+, Fe3+
Sc3+, Y3+, L3+
Why is the third ionization energy for calcium much larger than the first or second ionization energies?
Removing the third electron would result in the formation of an anion.
Core electrons would repel the electrons lost during the first and second ionizations.
Removing an electron from a noble gas electron configuration would take much more energy.
The first two electrons are in the d-subshell, thus easier to remove due to more shielding.
After the third ionization, calcium would become a nonmetal, therefore unstable.
Rank the following ions in order of increasing (that is, from smallest to largest) ionic radius.
In3+ < Sr2+ < Se2- < Rb+ < Br-
Br- < Rb+ < Sr2+ < Se2- < In3+
Br- < In3+ < Sr2+ < Rb+ < Se2-
In3+ < Sr2+ < Rb+ < Br- < Se2-
No trend can be predicted, since these elements are not from the same group or from the same period.
Which of the following concepts is NOT needed to solve the problem below?
"Calculate the volume occupied by 20 mmol of liquid nitrogen with a density of 808 g/L."
density
molar mass
mole
Avogadro's number
units of measure conversion
Which of the following would best describe the chemical bonding in solid potassium chloride, KCl?
electrostatic attractions between KCl molecules in a lattice
electron pairs shared by potassium and chlorine atoms
electron pairs shared by potassium and chlorine ions
electrostatic attractions between K+ and Cl- in a lattice
pairs of K+ and Cl- ions in a huge molecular structure
Write the Lewis structure of the N3- ion. Identify the total number of paired and unpaired valence
electrons, in that order.
2,3
3,2
8,0
7,5
5,0
In which sublevel (subshell) of the 4th main energy level (shell) would electrons always experience the
highest effective nuclear charge, Zeff?
s
p
d
f
Zeff does not depend on the energy sublevel, but only on the number of protons in the nucleus.
Elements from the same group have similar chemical properties because they have the same (a) .
[Kr] 5s2 4d10 5p5
Which type of element has this electron configuration?
halogen
noble gas
alkali metal
metalloid
transition metal
[Kr] 5s2 4d10 5p5
The element with this electron configuration has (a) valence electrons and 46 core electrons, in that
order.
Anions have a _______ charge and are ________ in volume than the atoms from which they formed.
positive; smaller
negative; smaller
positive; larger
negative; larger
zero; larger
Identify the electron configuration with the lowest first ionization energy.
1s2 2s2 2p6 3s1
1s2 2s2 2p6 3s2
1s2 2s2 2p6 3s2 3p1
1s2 2s2 2p6 3s2 3p2
1s2 2s2 2p6 3s2 3p3
Which shows correctly the dissociation of potassium hydrogen phosphate, K2HPO4, in water?
K+ + HPO4
-
2 K+ + HPO4
2-
K2+ + 2 HPO4
-
KH+ + PO4
3-
K2
2+ + HPO4
2-
Identify the set in which all atoms have a valence shell described by the general electron configuration
ns2 np4 (n represents the period number).
P, S, Cl
S, O, Te
Cr, Mo, W
Cs, Ba, La
B, Si, As
Which of the following statements is TRUE?
When a covalent bond forms, the energy of the two atoms decreases.
Valence electrons are the hardest to remove from an atom.
As atoms get closer together, their electrons attract each other.
Ionization energy increases when the effective nuclear charge decreases.
More shielded electrons can easier penetrate lower energy levels.
Which element has the largest value for the second ionization energy, IE2?
Al
Si
Ni
Mg
Na
Identify the element that has the ground-state electron configuration shown by the orbital diagram below:
carbon
nitrogen
fluorine
sulfur
oxygen
