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WorksheetsSenior 2 Periodic table
Total questions: 24
Worksheet time: 31mins
Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.
numbers, rows
masses, rows
masses, column
numbers, column
Metals (select all that apply)
are found on the right side of the periodic table.
are found on the left side of the periodic table.
are good conductors of heat and electricity.
are brittle.
are malleable and ductile.
Order the elements S, Cl, and F in terms of increasing ionization energy.
S, Cl, F
Cl, F, S
F, S, Cl
F, Cl, S
S, F, Cl
Order the elements S, Cl, and F in terms of increasing atomic radii.
S, Cl, F
Cl, F, S
F, S, Cl
F, Cl, S
S, F, Cl
List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.
Li<Na<C<O<F
Na<Li<C<O<F
F<O<C<Li<Na
Na<Li<F<O<C
Na<Li<C<F<O
Which element has the highest electronegativity?
Which of the atoms pictured would have the lower ionization energy and why?
Atom A because it it bigger
Atom A because the outer electrons are not "held" as tightly as those in atom B
Atom B because it is smaller
Atom B because the outer electrons have a greater attraction for the nucleus.
Organize the following ions from smallest to largest
P-3, S-2, Cl-
P-3 < S-2 < Cl-
P-3 < Cl- < S-2
Cl- < P-3 < S-2
Cl- < S-2 < P-3
Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the highest-energy photon.
n = 6 ¬ n = 1
n = 1 ¬ n = 6
n = 3 ¬ n = 6
n = 6 ¬ n = 3
The lines in the emission spectrum of hydrogen result from __________.
electrons given off by hydrogen as it cools
decomposing hydrogen atoms
electrons given off by hydrogen when it burns
energy given off in the form of visible light when an electron moves from a higher energy state to a lower energy state
__________-orbitals are spherically symmetrical
d
p
s
f
Which one of the following represents an acceptable possible set of quantum numbers (in the order n, l, ml, ms) for an electron in an atom?
2, 1, 0, 0
2, 2, 0, 1/2
2, 0, 2, +1/2
2, 0, 1, -1/2
2, 1, -1, 1/2
An example of an electron configuration of a transition metal is __________.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1
1s2 2s2 2p6 3s2 3p5
1s2 2s2 2p6 3s2 3p6 4s2 3d8
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
1s2 2s2 2p4 3s1
An example of an excited state electron configuration for fluorine is _________
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1
1s2 2s2 2p6 3s2 3p5
1s2 2s2 2p6 3s2 3p6 4s2 3d8
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
1s2 2s2 2p4 3s1
The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table
increase, increase
increase, decrease
decrease, increase
decrease, decrease
are completely unpredictable
Which ion in the isoelectronic series below has the smallest radius in a crystal?
O2-
N3-
Na+
Al3+
F-
The electron configuration of the atom that is expected to have the lowest first ionization energy is __________
[Kr] 5s1
[Ne] 3s2 3p5
[Ar] 4s2 3d10 4p4
[Ne] 3s2 3p6
[Ar] 4s1
The electron configuration of the atom that is expected to have the highest first ionization energy is __________
[Kr] 5s1
[Ne] 3s2 3p5
[Ar] 4s2 3d10 4p4
[Ne] 3s2 3p6
[Ar] 4s1
__________ have the lowest first ionization energies of the groups listed.
Transition elements
Halogens
Alkaline earth metals
Alkali metals
Noble Gases
Which of the following ground-state electron configurations represents the atom that has the lowest first-ionization energy?
1s2 2s1
1s2 2s2 2p6 3s1
1s2
1s2 2s2 2p6
