The primary reason ionization energy increases from left to right across a period is:

Increasing effective nuclear charge (Zeff).

Increasing number of electron shells.

Compared to a neutral sulfur atom (S), the sulfide ion (S2–) is:

Larger because it gained electrons, increasing electron-electron repulsion.

Smaller because it lost electrons.

Smaller because its nuclear charge is effectively greater.

The concept of resonance is used when:

B) One Lewis structure cannot accurately represent the true electron distribution.

A) A molecule has only single bonds.

C) The central atom has more than an octet of electrons.

D) A molecule is perfectly symmetrical.

Which of the following molecules is nonpolar?

BF3 (Boron trifluoride, trigonal planar)

Even if the bonds within a molecule are polar, the molecule itself can be nonpolar if:

The molecule has a symmetrical shape that causes the bond dipoles to cancel.

The molecule contains hydrogen.

The central atom is in the third period or below.

Hydrogen bonding occurs when hydrogen is bonded to:

A highly electronegative atom like Nitrogen, Oxygen, or Fluorine.

Carbon or another hydrogen atom.

Which statement best describes why CH4 has a much lower boiling point than NH3?

CH4 has weaker London dispersion forces than NH3, which has hydrogen bonding.

CH4 has stronger hydrogen bonding than NH3.

CH4 has a larger molecular mass than NH3.

Which of the following is NOT a typical property of covalent molecular compounds?

Good conductors of electricity in the solid state.

Low melting and boiling points.

Often gases or liquids at room temperature.

Chem practice final 2

Authored by Cesar Segundo

Science

11th Grade

NGSS covered

Used 25+ times

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MULTIPLE CHOICE QUESTION

2 mins • 1 pt

What is the correct noble gas shorthand electron configuration for a neutral atom of Calcium (Ca)?

[Ne]3s2

[Ar]4s2

[Kr]5s2

[Ar]3d2

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

An atom has the electron configuration 1s22s22p63s23p64s13d10. Which element is this?

Potassium (K)

Copper (Cu)

Zinc (Zn)

Nickel (Ni)

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

How many valence electrons does a neutral atom of Bromine (Br) have?

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

The Pauli Exclusion Principle states that:

Electrons fill orbitals of the lowest energy first.

Electrons occupy orbitals singly before pairing.

No two electrons in an atom can have the same four quantum numbers (or an orbital can hold max 2 electrons with opposite spins).

Only two electrons can occupy an s orbital.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

What is the electron configuration of a K+ ion?

1s22s22p63s23p5

1s22s22p63s23p64s1

1s22s22p63s23p6

1s22s22p63s23p44s2

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Which of the following subshells has the highest energy?

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Which of the following elements has the smallest atomic radius?

Beryllium (Be)

Magnesium (Mg)

Calcium (Ca)

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Chem practice final 2

What is the correct noble gas shorthand electron configuration for a neutral atom of Calcium (Ca)?

An atom has the electron configuration 1s22s22p63s23p64s13d10. Which element is this?

How many valence electrons does a neutral atom of Bromine (Br) have?

The Pauli Exclusion Principle states that:

What is the electron configuration of a K+ ion?

Which of the following subshells has the highest energy?

Which of the following elements has the smallest atomic radius?

Which of these elements has the lowest first ionization energy?

Arrange the following elements in order of increasing electronegativity: P, Na, Cl, Al.

Which of the following ions is largest?

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