Learning Modules 13-14

What is the effective nuclear charge (ENC) experienced by a 1s electron and a 2p electron, respectively, in the F^-1 anion?

• 9, 7

• 2, 9

• 10, 7

• 10, 2

Tags

NGSS.HS-PS1-1

What is the full electronic configuration for neutral chlorine?

• 1s²2s²2p⁶3s²3p⁵

• 1s²2s²2p⁶3s⁷

• 1s²2s²2p⁶3s²3p⁶

• 1s²2s²2p⁶3s²3d¹⁰3p⁵

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Diamagnetic substances....

• have no unpaired electrons and are weakly repelled by a magnetic field.

• have no unpaired electrons and are weakly attracted by a magnetic field.

• have unpaired electrons and are weakly repelled by a magnetic field.

• have unpaired electrons and are weakly attracted by a magnetic field.

Tags

NGSS.HS-PS1-1

Which of the following statements about the periodic trend of atomic radius is/are true?

I. Atomic radius decreases from left to right across a period because Zeff increases.
II. Atomic radius increases from left to right across a period because the number of valence
electrons increases.
III. Atomic radius increases from top to bottom in a group because the number of electron
shells increases.

• II only

• I and III only

• I only

• II and III only

Tags

NGSS.HS-PS1-1

The energy needed to remove electrons from an atom is called

• bonding energy

• ionization energy

• valence energy

• network energy

Tags

NGSS.HS-PS1-1

What is the correct order of increasing electronegativity?

• O, C, N, S, P, Si, F

• Si, P, S, C, N, O, F

• F, O, N, C, S, P, Si

• F, Si, P, S, N, C, O

The maximum number of electrons that the second energy level of an atom can hold is

• 8

• 10

• 32

• 2

An electron in a 3d orbital could have which of the following quantum numbers?

• n = 2; ℓ = 2; m ℓ = 2

• n = 3; ℓ = 2; m ℓ = 0

• n = 3; ℓ = 3; m ℓ = 1

• n = 3; ℓ = 2; m ℓ = −3

Which statement gives the name and correct principle which is used to determine the arrangement of electrons in degenerate orbitals when writing electron configurations?

• Mendeleev: leave unoccupied spaces in the degenerate orbitals in case we discover any new orbitals.

• Aufbau principle: fill all degenerate orbitals first, then fill in any higher or lower energy orbitals which are not degenerate.

• Hund’s rule: put one electron in each degenerate orbital first, then add one more electron with an opposite spin to each orbital.

• Pauli Principle: only put one electron in any orbital.