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WorksheetsPeriodic Trends
Total questions: 20
Worksheet time: 5hrs 0mins
Name
Class
Date
1.
Which of the following pairs has the highest ionization energy?
a)
Li and Na
b)
P and S
c)
N and O
d)
Fe and Co
2.
Which of the following elements in the periodic table have the highest first ionization energies?
a)
transition elements
b)
alkaline earth metals
c)
alkali metals
d)
noble gas elements
3.
Which of the following elements has the smallest radius?
a)
Mg
b)
Al
c)
Si
d)
K
4.
Which of the following atoms or ions is the largest in diameter?
a)
C
b)
P
c)
Te2-
d)
Se
5.
Which of the following elements has an electron affinity that is close to zero?
a)
nitrogen
b)
phosphorus
c)
boron
d)
oxygen
6.
Which of the following sets of elements are arranged in order of INCREASING metallic radii?
a)
Cs < Ba < La < Hf < Ta
b)
Al < Si < P < S < Cl
c)
Be < Mg < Ca < Sr < Ba
d)
Rb < K < Na < Li < H
7.
Why do noble gases have the highest first ionization energies?
a)
The principal quantum number increases left to right across the periodic table.
b)
The effective nuclear charge is low.
c)
The electron affinity is zero.
d)
An electron is harder to remove from a noble gas due to it being tightly bound by the inner nucleus.
8.
Variation of Ionization with Atomic Number
The picture shows the plot of the variation of the first ionization energy with the atomic number of the periodic elements. The ionization energies of boron, oxygen, aluminum and sulfur dips because
The picture shows the plot of the variation of the first ionization energy with the atomic number of the periodic elements. The ionization energies of boron, oxygen, aluminum and sulfur dips because
a)
the nuclear charge increases with atomic number.
b)
the ionic radii decreases from B to Al and O to S.
c)
less energy is required to remove a "p" electron than an "s" electron.
d)
these elements have stable electron configurations.
9.
Which periodic group exhibits BOTH high ionization energies and large negative electron affinities?
a)
alkali metals
b)
transition elements
c)
inert gases
d)
halogens
10.
Periodic Table of Elements
The International Union of Pure and Applied Chemistry (IUPAC) have recently announced they have added four of the newest elements: Nihonium (Nh-113), Moscovium (Mc-115), Tennessine (Ts-117), Organessum (Og-118).
In which area of the periodic table do these elements belong?
The International Union of Pure and Applied Chemistry (IUPAC) have recently announced they have added four of the newest elements: Nihonium (Nh-113), Moscovium (Mc-115), Tennessine (Ts-117), Organessum (Og-118).
In which area of the periodic table do these elements belong?
a)
The sixth row of the Periodic Table.
b)
The seventh row of the Periodic Table.
c)
Actinides group.
d)
Lanthanides group.
11.
Which of the following properties are characteristic of nonmetals?
a)
They are malleable and ductile.
b)
They are poor conductors of electricity.
c)
They exist as extended planes of atoms.
d)
They are typically solids at room temperature.
12.
Despite the fact that lithium is prescribed in the form of lithium salt for the treatment of bipolar disorder, the element lithium is unsuitable for human consumption due to its violent reaction with water.
What could be a possible reason for its reaction with water?
What could be a possible reason for its reaction with water?
a)
Low atomic mass.
b)
Low ionization energy.
c)
Oxidation state of +1.
d)
High electron affinity.
13.
Which of the elements listed have the largest ionization energy and highest electronegativity?
a)
F
b)
Cl
c)
Br
d)
I
14.
Which of the following have properties of both metals and nonmetals?
a)
C, Si, Ge, Sn, Pb
b)
Na, Mg, Al, Si, P
c)
Al, B, N, S, P
d)
Si, Ge, B, As, Sb
15.
Which of the following electron configurations represents an element with the largest atomic radius?
a)
1s22s22p63s1
b)
1s22s22p63s23p64s2
c)
1s22s22p63s23p63d104s1
d)
1s22s22p63s23p2
16.
Which of the following statements is FALSE about the Group 15 elements in the Periodic Table?
(shown L to R in the photo is: nitrogen, phosphorus, arsenic, antimony, bismuth)
(shown L to R in the photo is: nitrogen, phosphorus, arsenic, antimony, bismuth)
a)
The metallic character of the elements increases down a group.
b)
The elements stored in water are highly reactive in air.
c)
The atoms at the top of this group lose electrons less readily than those at the bottom of the group.
d)
Bismuth is a nonmetal.
17.
Which of the following physical properties can exist as both positive and negative quantities?
a)
Ionization energy.
b)
Electron affinity.
c)
Atomic radius.
d)
Electronegativity.
18.
Arrange the following isoelectronic ions in INCREASING order of atomic radius.
a)
S2- < Cl- < K+ < Ca2+ < Sc3+
b)
K+ < Ca2+ < Sc3+ < Cl- < S2-
c)
Sc3+ < Ca2+ < K+ < Cl- < S2-
d)
Cl- < S2- < K+ < Ca2+ < Sc3+
19.
Electron affinities of Group 2 elements have positive electron affinity (EA) values (in kJ/mol) because
a)
the energy is given up by the system to the surroundings when an electron is added to the atom.
b)
they have little tendancy to add an electron to the atom to form a negative ion.
c)
they are alkaline metals.
d)
they have a greater tendency to lose an electron to form a cation.
20.
Two elements (A and B) have the electron configurations below:
A: 1s22s22p63s23p64s1
B: 1s22s22p63s23p4
In addition, the table shows different physical properties of these two elements. The data was mixed up in a computer crash, thus the values are not in the same order as the electron configurations, nor are values associated by column.
Help put the data back correctly.
Physical Properties of Periodic Elements
1st & 2nd Ionization Energies (IE) (kJ/mol)
786.4 1577
418 3051
Ionic Radius (IR in nm) 0.113 0.041
Electron Affinity (EA in kJ/mol) -133.6 -48.36
Electronegativity (EA) 1.9 0.82
A: 1s22s22p63s23p64s1
B: 1s22s22p63s23p4
In addition, the table shows different physical properties of these two elements. The data was mixed up in a computer crash, thus the values are not in the same order as the electron configurations, nor are values associated by column.
Help put the data back correctly.
Physical Properties of Periodic Elements
1st & 2nd Ionization Energies (IE) (kJ/mol)
786.4 1577
418 3051
Ionic Radius (IR in nm) 0.113 0.041
Electron Affinity (EA in kJ/mol) -133.6 -48.36
Electronegativity (EA) 1.9 0.82
a)
A = potassium: (IE = 418, 3051; IR = .041; EA = -48.36; EN = 0.82)
B = silicon: (IE = 786.4, 1577; IR = .133; EA = -133.6; EN = 1.9)
B = silicon: (IE = 786.4, 1577; IR = .133; EA = -133.6; EN = 1.9)
b)
A = potassium: (IE = 786.4, 1577; IR = 0.041; EA = -48.36; EN = 0.82)
B = silicon: (IE = 418, 3051; IR = 0.133; EA = -133.6; EN = 1.9)
B = silicon: (IE = 418, 3051; IR = 0.133; EA = -133.6; EN = 1.9)
c)
A = potassium: (IE = 418, 3051; IR = .133; EA = -48.36; EN = 0.82)
B = silicon: (IE = 786.4, 1577; IR = .041; EA = -133.6; EN = 1.9)
B = silicon: (IE = 786.4, 1577; IR = .041; EA = -133.6; EN = 1.9)
d)
A = potassium: (IE = 786.4, 1577; IR = .041; EA = -48.36; EN = 1.9)
B = silicon: (IE = 418, 3051; IR = .133; EA = -133.6; EN = 0.82)
B = silicon: (IE = 418, 3051; IR = .133; EA = -133.6; EN = 0.82)
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