AP Chemistry: 1.7 Periodic Trends- Exam Style questions with Answer- MCQ

AP PhysicsAP Calculus AP ChemistryAP Biology

Question

The atomic radii of the elements in the nitrogen group in the periodic table are given in the table above. Which of the following best helps explain the trend of increasing atomic radius from $N$ to $Bi$ ?

A The number of particles in the nucleus of the atom increases.

B The number of electrons in the outermost shell of the atom increases.

C The attractive force between the valence electrons and the nuclei of the atoms decreases.

D The repulsive force between the valence electrons and the electrons in the inner shells decreases.

▶️Answer/Explanation

Ans:C Going down the group, the net attraction of the valence electrons for the nucleus decreases; thus the valence electrons maintain a greater average distance from the nucleus.

Question

Which of the following best helps to explain why the atomic radius of $K$ is greater than that of $Br$ ?

A The first ionization energy of

K

is higher than that of

Br

B The valence electrons in $K$ are in a higher principal energy level than those of $Br$ .

C In the ground state, an atom of $K$ has fewer unpaired electrons than an atom of $Br$ has.

D The effective nuclear charge experienced by valence electrons is smaller for

K

than for

Br

▶️Answer/Explanation

Ans: D Because the effective nuclear charge of $K$ is smaller than that of $Br$ , the attraction between its valence electron and the nucleus is less than the attraction between the valence electrons in $Br$ and the nucleus.

Question

Which of the following best helps explain why the first ionization energy of $K$ is less than that of $Ca$ ?

A The electronegativity of

K

is greater than that of

Ca

B The atomic radius of the

K

atom is less than that of the

Ca

atom.

C The valence electron of

K

experiences a lower effective nuclear charge than the valence electrons of

Ca

D The nucleus of the

K

atom has fewer neutrons, on average, than the nucleus of the

Ca

atom has.

▶️Answer/Explanation

Ans: C The amount of energy required to remove the electron \( $I E sub 1$ ) will depend on the strength of the attractive force between the electron and the nucleus, as predicted by Coulomb’s law.

Question

Which of the following correctly identifies which has the higher first-ionization energy, Cl or Ar and supplies the best justification?

(A) CI, because of its higher electronegativity

(B) Cl. because of its higher electron affinity

(C) Ar, because of its completely filled valence shell

(D) Ar, because of its higher effective nuclear charge

▶️Answer/Explanation

Answer/Explanation

Ans:D

Question

The table above shows the first ionization energy and atomic radius of several elements. Which of the following best helps to explain the deviation of the first ionization energy of oxygen from the overall trend?

(A)The atomic radius of oxygen is greater thalh the atomic radius of fluorine.

(B)The atomic radius of oxygen is less than the atomic radius of nitrogen.

(C)There is repulsion between paired electrons in oxygen’s 2P orbitals.

(D)There is attraction between paired electrons in oxygen’s 2P orbitals.

▶️Answer/Explanation

Ans:C

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