Question 1

An element with the electron configuration [noble gas]ns²(n - 1)d⁸ has ________ valence electrons. A) 2 B) 6 C) 8 D) 10 E) None of these choices is correct.

Accepted Answer

The answer of An element with the electron configuration [noble...

Question 2

How many valence electrons does a tin (Sn) atom have?
A) 2
B) 4
C) 14
D) 36
E) 50

Accepted Answer

Tin (Sn) is in group 14 of the periodic table, which means it has 4 valence electrons.

Question 3

How many valence electrons does a carbon atom have?
A) 1
B) 2
C) 3
D) 4
E) 6

Accepted Answer

Carbon has 4 valence electrons, meaning it has the capacity to form 4 covalent bonds with other atoms.

Question 4

Consider the element with the electron configuration [Xe]6s²4f⁷. This element is A) a halogen. B) a lanthanide element. C) a nonmetal. D) an actinide element. E) a noble gas.

Accepted Answer

The electron configuration [Xe]6s²4f⁷ corresponds to a lanthanide element, specifically europium (Eu), which is part of the lanthanide series.

Question 5

An element with the electron configuration [noble gas]ns²(n - 1)d¹⁰^np³ has ________ valence electrons. A) 2 B) 3 C) 5 D) 10 E) 15

Accepted Answer

To determine the valence electrons, we look at the outermost energy level, which is the n level. Counting the electrons in the ns, np, and nd subshells of the n level gives us the number of valence electrons.

In this case, the outermost energy level is n, and there are 5 electrons in the ns, np, and nd subshells of the n level. Therefore, the element has 5 valence electrons.

Question 6

Which of these atoms has the smallest radius?
A) Al
B) P
C) As
D) Te
E) Na

Accepted Answer

Phosphorus (P) has the smallest atomic radius among the options given. Atomic radius generally decreases across a period from left to right due to the increase in nuclear charge, which pulls the electrons closer to the nucleus. Phosphorus is to the right of Aluminum and Sodium in the same period, indicating a smaller atomic radius. Additionally, as you move down a group, atomic radius increases due to the addition of electron shells, making Phosphorus smaller than Arsenic and Tellurium, which are below it in the same group.

Question 7

The energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?
A) Larger nuclear charge lowers energy; more electrons in an orbital lowers energy.
B) Larger nuclear charge lowers energy; more electrons in an orbital increases energy.
C) Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy.
D) Smaller nuclear charge lowers energy; more electrons in an orbital increases energy.
E) None of these statements is generally correct.

Accepted Answer

The larger nuclear charge attracts electrons more strongly, thus lowering their energy. However, electron-electron repulsion increases as more electrons occupy an orbital, causing higher energy.

Question 8

How does atomic radius change as you move across the periodic table?
A) Atomic radius decreases moving from left to right across a period and increases from top to bottom.
B) Atomic radius increases moving left to right across a period and decreases from top to bottom.
C) Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy.
D) Atomic radius increases diagonally across the periodic table.
E) None of the answers is correct.

Accepted Answer

Atomic radius decreases as you move from left to right across a period due to the increase in nuclear charge, which pulls electrons closer to the nucleus. It increases from top to bottom within a group because each row adds a new electron shell, making the atom larger.

Question 9

Which one of these ions has the smallest radius? A) Cl^- B) K⁺ C) S^2- D) Na⁺ E) O^2-

Accepted Answer

The answer of Which one of these ions has the...

Question 10

Consider the element with the electron configuration [Kr]5s²4d¹⁰5p⁵. This element is A) a halogen. B) a transition metal. C) an alkali metal. D) an actinide element. E) a noble gas.

Accepted Answer

The electron configuration [Kr]5s²4d¹⁰5p⁵ corresponds to an element in Group 17 of the periodic table, which are known as halogens.

Question 11

An element with the general electron configuration for its outermost electrons of ns²^np¹ would be in which element group? A) 2A B) 3A C) 4A D) 5A E) 8A

Accepted Answer

The given electron configuration simplifies to ns^2 np^1, indicating that the element has three electrons in its outermost shell (two in the s orbital and one in the p orbital). This configuration corresponds to the elements in group 3A of the periodic table.

Question 12

Arrange P, S, and O in order of increasing atomic radius.
A) S < O < P
B) P < S < O
C) O < S < P
D) O < P < S
E) The answer cannot be determined from the data given.

Accepted Answer

Atomic radius generally increases as you move down a group and from right to left across a period. Oxygen (O) is to the right of sulfur (S) and phosphorus (P) in period 3, so it has the smallest atomic radius. Sulfur has one more energy level than oxygen, so it has a larger atomic radius. Phosphorus has two more energy levels than oxygen, so it has the largest atomic radius of the three. Therefore, the order is O < S < P.

Question 13

Each of the noble gases has a completely filled p subshell except for which one?
A) Xenon
B) Neon
C) Radon
D) Argon
E) Helium

Accepted Answer

Helium is the exception because it has a completely filled s subshell (1s^2) but does not have a p subshell, as it is in the 1s orbital, which is before the start of the p block elements in the periodic table.

Question 14

Which of the elements listed below has the greatest atomic radius?
A) B
B) Al
C) S
D) P
E) Si

Accepted Answer

Atomic radius increases as you move down a group and from right to left across a period. Therefore, among the given elements, Al has the greatest atomic radius.

Question 15

In what group of the periodic table is the element with the electron configuration [Ar]4s²3d¹⁰4p³? A) 1A B) 2A C) 3A D) 4A E) 5A

Accepted Answer

The given electron configuration is not standard notation and seems to contain typographical errors. However, interpreting it as [Ar] 4s^2 3d^10 4p^3 suggests the element is from group 5A (15) of the periodic table, as elements in this group have five electrons in their outermost p orbital, which corresponds to the configuration ending in 4p^3.

Question 16

The effective nuclear charge for an atom is less than the actual nuclear charge due to
A) shielding.
B) penetration.
C) paramagnetism.
D) electron-pair repulsion.
E) relativity.

Accepted Answer

The effective nuclear charge is the net positive charge experienced by an electron in an atom. It is less than the actual nuclear charge due to shielding, which is caused by the presence of other electrons in the atom that partially cancel the attraction between the nucleus and the electron in question. Shielding occurs when electrons in inner energy levels partially block the attraction between the positively charged nucleus and the outer electron, reducing the effective nuclear charge.

Question 17

The general electron configuration for atoms of the halogen group is A) ns²^np⁶^. B) ns²^np⁵. C) ns²^np⁶ (n - 1)d⁷. D) ns¹. E) ns²^np⁷.

Accepted Answer

The general electron configuration for atoms of the halogen group is ns²np⁵. Option B follows this pattern and is the correct choice. The other options have incorrect subshells or an incorrect number of electrons.

Question 18

Which of these atoms has the largest radius?
A) B
B) Ga
C) Br
D) Si
E) Cl

Accepted Answer

As we move down a group on the periodic table, the atomic radius tends to increase because the number of energy levels increases. Ga is located below B in the same group, so it has a larger atomic radius than B. Br, Cl, and Si are all located in different periods than B and Ga, so their atomic radii cannot be accurately compared without further information.

Question 19

The general electron configuration for noble gas atoms is A) ns²^np⁶. B) ns²^np⁵. C) ns²^np⁴. D) ns²^np³. E) ns².

Accepted Answer

Noble gases have a full outer shell, which is represented by the electron configuration ns²np⁶ for elements in periods 2 and above.

Question 20

Consider the element with the electron configuration [Kr]5s²4d⁷. This element is A) a halogen. B) a transition metal. C) a nonmetal. D) an actinide element. E) a noble gas.

Accepted Answer

The given electron configuration is incorrectly formatted with characters like "S" and "U" that don't belong in electron configurations. However, the correct interpretation seems to aim towards a transition metal, given the presence of a "4d" subshell being partially filled, which is characteristic of transition metals. Transition metals are defined by having an incomplete d subshell in one or more of their oxidation states.

Quiz 7: Electron Configuration and the Periodic Table

An element with the electron configuration [noble gas]ns²(n - 1) d⁸ has ________ valence electrons.

How many valence electrons does a tin (Sn) atom have?

How many valence electrons does a carbon atom have?

Consider the element with the electron configuration [Xe]6s²4f⁷. This element is

An element with the electron configuration [noble gas]ns²(n - 1) d¹⁰^np³ has ________ valence electrons.

Which of these atoms has the smallest radius?

The energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

How does atomic radius change as you move across the periodic table?

Which one of these ions has the smallest radius?

Consider the element with the electron configuration [Kr]5s²4d¹⁰5p⁵. This element is

An element with the general electron configuration for its outermost electrons of ns²^np¹ would be in which element group?

Arrange P, S, and O in order of increasing atomic radius.

Each of the noble gases has a completely filled p subshell except for which one?

Which of the elements listed below has the greatest atomic radius?

In what group of the periodic table is the element with the electron configuration [Ar]4s²3d¹⁰4p³?

The effective nuclear charge for an atom is less than the actual nuclear charge due to

The general electron configuration for atoms of the halogen group is

Which of these atoms has the largest radius?

The general electron configuration for noble gas atoms is

Consider the element with the electron configuration [Kr]5s²4d⁷. This element is