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Electron Configuration and Periodic Table Trends Flashcards | StudBud
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Electron Configuration and Periodic Table Trends
Electron Configuration and Periodic Table Trends
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1
What is the correct configuration for Cl 1-
[Ne] 3s2 3p6
[Ar] 3s2 3p6
1s2 2s2 2p6 3s2 3p5
[Ne] 3s2 3p5
2
Electron affinity describes
the distance between the nucleus of the atom and the outermost electron
the change in energy of a neutral atom when an electron is added
the amount of energy required to remove an electron from an atom
the tendency of an atom to attract a shared pair of electrons
3
Which of the following would have the largest radius?
Mg 2+
F -
Ne
Na +
4
This group has some of the highest ionization energies, but is an exception to electronegativity trends
Alkali Metals
Metalloids
Halogens
Noble Gases
5
Which of the following elements will form an ion larger than the parent atom?
Aluminum
Sulfur
Calcium
Potassium
6
What rule is broken in this configuration?
Aufbau
None
Pauli
Hund
7
Which correctly orders these elements from lowest to greatest electronegativity?
Ni < Sr < N < B
Sr < Ni < B < N
N < B < Ni < Sr
B < N < Sr < Ni
8
Cations are
often non-metals and smaller than the parent atom
often metals and smaller than the parent atom
often non-metals and smaller than the parent atom
often metals and larger than the parent atom
9
Which of the following would have the largest radius?
F
K
Li
Br
10
How many electrons are present in the following configuration? 1s2 2s2 2p6 3s2 3p5
11
7
17
15
11
Which of the following explains decreasing radius trends within a period?
Higher effective nuclear charge
More electron shells
Lower effective nuclear charge
Fewer electron shells
12
Electron affinity increases
up and left
up and right
down and right
down and left
13
Which of the following would have the smallest radius?
Kr
Sr 2+
Br -
Rb +
14
Atoms with low electron affinity have large radii?
False
True
15
What rule is broken here?
Pauli
None
Hund
Aufbau
16
Why is the bottom electron configuration incorrect?
electrons in an orbital share the same spin direction
both configurations are correct
both of these
electrons are paired when there are still empty p orbitals
17
Inner transition metals are associated with
the d-block
the s-block
the p-block
the f-block
18
What is the configuration for Cobalt?
1s22s22p62d103s2
1s22s22p63s23p64s23d7
1s22s22p63s23p64s24p65s1
1s22s22p63s23p63d9
19
Which group of elements/ions could this electron configuration refer to? 1s2 2s2 2p6 3s2 3p1
B, C +, Be -
Al, Si -, Mg +
Al, Si +, P 2+
Al, B, Ga
20
What is the noble gas configuration for Potassium?
[Kr] 4s1
[Ar] 4s1
[Kr] 5s1
[Ne] 3s1
21
Atomic radius decreases
As group number increases, and period number decreases
As group number decreases, and period number increases
As group and period number increases
As group and period number decreases
22
What explains the large increases in ionization energy shown in this image?
All of these
Electrons removed are held less tightly
Electrons removed are coming from lower shells
Electrons removed are coming from higher shells
23
Which is most likely to lose an electron?
Calcium
Potassium
Selenium
Bromine
24
Which of the following are isoelectronic?
K -, Ar, F+
Sr 2+, Kr, Br -
Ar, Kr, Ne
Na +, O -, Ne
25
Identify the neutral element with the following electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
Si
Ge
Cu
Ca
26
How many electrons can p orbitals hold?
3
5
10
6
27
The fourth electron shell can hold
8 electrons
32 electrons
2 electrons
18 electrons
28
An element that has a large increase in ionization energy between the second and third electron removed is most likely a
period 3 element
group 3 element
group 2 element
period 2 element
29
Which of the following elements would have the highest first ionization energy?
Sulfur
Carbon
Silicon
Oxygen
30
Which of the following explains Ionization energy increases in a group?
Increased electron distance from the nucleus
Higher effective nuclear charge
Decreased electron distance from the nucleus
Lower effective nuclear charge
