Question

1. examine the following outer electron configuration and choose the correct location of the element it represents in the periodic table: 5s2

a. row 7 column 4
c. row 5 column 2
b. row 4 column 7
d. row 5 column 9

1. the element from question 10 is in

a. period 5, alkali metal
c. period 5, halogen
b. period 4, halogen
d. period 5, transitional metal

1. sodium and potassium have similar properties because they have the same:

a. atomic radius
c. ionization energy
b. number of valence electrons
d. electronegativity

1. the likeliest charge an atom with 2 valence electrons would develop

a. 2+
b. 6+
c. 2-
d. 6-

1. the likeliest charge an atom with 6 valence electrons will develop

a. 2+
b. 6+
c. 2-
d. 6-

1. how many electrons are in the highest occupied energy level of a sodium?

a. 1
b. 2
c. 3
d. 6

1. what is the maximum number of electrons that can occupy the 5p sublevel?

a. 2
b. 4
c. 6
d. 8

1. how many orbitals in the 4p sublevel?

a. 1
b. 2
c. 3
d. 4

1. what is the maximum number of electrons that can occupy the 4th energy level?

a. 9
b. 18
c. 20
d. 32

1. which is the symbol of the element whose electron configuration is 1s²2s²2p⁶3s²3p⁶4s²

a. ca
b. li
c. rb
d. ar

1. elements tend to gain or lose electrons in order to acquire the electron configuration of a:

a. halogen
b. transition metal
c. noble gas
d. nonmetal

Explanation:

Step1: Analyze electron - configuration for location

The outer - electron configuration is \(5s^{2}\). The principal quantum number \(n = 5\) indicates the row (period) is 5, and the number of electrons in the outermost \(s\) - subshell is 2, so the column (group) is 2.

Step2: Identify element type from electron - configuration

An element with outer - electron configuration \(5s^{2}\) is in period 5. Elements in group 2 are alkaline earth metals, not alkali metals, halogens, or transition metals.

Step3: Recall periodic - trend property similarity

Sodium (\(Na\)) and potassium (\(K\)) are in the same group (group 1). Elements in the same group have the same number of valence electrons, which gives them similar chemical properties.

Step4: Determine charge for 2 valence electrons

An atom with 2 valence electrons will lose these 2 electrons to achieve a stable electron configuration, forming a \(2+\) ion.

Step5: Determine charge for 6 valence electrons

An atom with 6 valence electrons will gain 2 electrons to achieve a stable electron configuration (octet), forming a \(2-\) ion.

Step6: Find electrons in sodium's highest occupied energy level

Sodium (\(Na\)) has an electron - configuration of \(1s^{2}2s^{2}2p^{6}3s^{1}\). The highest occupied energy level is \(n = 3\), and there is 1 electron in the \(3s\) orbital.

Step7: Recall electron capacity of \(5p\) sublevel

The \(p\) sublevel has 3 orbitals, and each orbital can hold a maximum of 2 electrons. So, the \(5p\) sublevel can hold \(2\times3=6\) electrons.

Step8: Recall number of orbitals in \(4p\) sublevel

The \(p\) sublevel always has 3 orbitals, regardless of the principal quantum number \(n\). So, the \(4p\) sublevel has 3 orbitals.

Step9: Calculate electrons in 4th energy level

The formula to calculate the number of electrons in an energy level \(n\) is \(2n^{2}\). For \(n = 4\), \(2\times4^{2}=2\times16 = 32\) electrons.

Step10: Identify element from electron - configuration

The electron - configuration \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}\) corresponds to calcium (\(Ca\)).

Step11: Determine stable electron - configuration goal

Elements tend to gain or lose electrons to acquire the electron - configuration of a noble gas, which has a stable octet (or duet for \(n = 1\)) of electrons.

Answer:

1. c. row 5 column 2
2. a. period 5, alkali metal
3. b. number of valence electrons
4. a. \(2+\)
5. c. \(2-\)
6. a. 1
7. c. 6
8. c. 3
9. d. 32
10. a. \(Ca\)
11. c. noble gas