Chemistry Unit Review

Arrange these elements in order of increasing electronegativity: antimony, fluorine, indium, selenium

• antimony, fluorine, indium, selenium

• indium, selenium, antimony, fluorine,

• indium, fluorine, selenium antimony

• indium, antimony, selenium, fluorine

Arrange these elements in order of increasing electronegativities: francium, gallium, germanium, phosphorus, zinc

• phosphorus, zinc, francium, gallium, germanium

• francium, gallium, germanium, phosphorus, zinc

• phosphorus, francium, gallium, germanium zinc

• francium, zinc, gallium, germanium, phosphorus

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Calculate ΔEN for Pb-S

• 1.1

• -0.1

• 0.1

• 3.7

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Calculate ΔEN for Na-Br

• 1.9

• 0.9

• 2.8

• 1.0

Which type of bond is created between C-N?

• Polar Covalent

• Non-polar Covalent

• Ionic

• Metallic

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which type of bond is created between Na-I?

• Polar Covalent

• Non-polar Covalent

• Ionic

• Metallic

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Based on electronegativies, which of the following would you expect to be most ionic?

• N₂

• NaF

• CO

• there is no way to tell

The Lewis structure of N₂H₂ shows __________.

• a nitrogen-nitrogen triple bond

• a nitrogen-nitrogen single bond

• each nitrogen has one lone pair

• each nitrogen has two lone pairs

• each hydrogen has one lone pair

In the nitrite ion (NO₂^-), __________.

• both bonds are single bonds

• both bonds are double bonds

• both bonds are the same because of resonance

• there are 20 valence electrons

• there is one single and one double bond

A valid Lewis structure of _______ cannot be drawn without violating the octet rule.

• NF₃

• IF₃

• PF₃

• SbF₃

• SO₄^2-