CART - Chemistry Acceleration Readiness Atomic Structure and Periodicity Questions and Answers

Question 1

Which of the following sets of quantum numbers (n, l, m_l, m_s) is invalid for an electron in an atom?

Accepted Answer

4, 3, -4, +1/2

Answer

The magnetic quantum number, m_l, can only have integer values from -l to +l. In the set (4, 3, -4, +1/2), l=3, so the possible values for m_l are -3, -2, -1, 0, 1, 2, and 3. The value -4 is not allowed, making this set of quantum numbers invalid.

Question 2

An atom has an atomic number of 15 and a mass number of 31. How many protons, neutrons, and electrons does a neutral atom of this element have?

Accepted Answer

15 protons, 16 neutrons, 15 electrons

Answer

The atomic number (Z) is equal to the number of protons. For a neutral atom, the number of electrons is equal to the number of protons. The mass number (A) is the sum of protons and neutrons. Therefore, protons = 15, electrons = 15, and neutrons = Mass Number - Protons = 31 - 15 = 16.

Question 3

Consider the elements Fluorine (F), Carbon (C), and Oxygen (O). Which of the following correctly lists these elements in order of increasing atomic radius?

Accepted Answer

F, O, C

Answer

Atomic radius generally decreases from left to right across a period in the periodic table. This is because as the atomic number increases across a period, the effective nuclear charge increases, pulling the electron shells closer to the nucleus. Fluorine, Oxygen, and Carbon are all in Period 2. Carbon (Group 14) is furthest to the left, followed by Oxygen (Group 16), and then Fluorine (Group 17). Therefore, the order of increasing atomic radius is F < O < C.

Question 4

What is the ground-state electron configuration for a sulfide ion (S²⁻)?

Accepted Answer

1s²2s²2p⁶3s²3p⁶

Answer

A neutral sulfur atom (S) has an atomic number of 16, so its electron configuration is 1s²2s²2p⁶3s²3p⁴. The sulfide ion (S²⁻) has gained two electrons. These two electrons are added to the outermost shell, which is the 3p subshell. This fills the 3p subshell completely, resulting in the electron configuration 1s²2s²2p⁶3s²3p⁶, which is isoelectronic with the noble gas Argon.

Question 5

Which of the following statements best describes the trend of first ionization energy on the periodic table?

Accepted Answer

It decreases down a group and increases from left to right across a period.

Answer

First ionization energy is the energy required to remove the outermost electron from a neutral atom. It decreases down a group because the valence electrons are in higher energy levels, are farther from the nucleus, and experience more shielding, making them easier to remove. It increases from left to right across a period because the increasing effective nuclear charge holds the electrons more tightly, requiring more energy to remove one.

CART - Chemistry Acceleration Readiness Test Practice Test

CART - Chemistry Acceleration Readiness Test Practice Test

CART - Chemistry Acceleration Readiness Atomic Structure and Periodicity Questions and Answers