LHHS FPFSA Chapter 8

What is an example of a diatomic molecule

• H₂

• HBr

• H₂O

Molecular compounds tend to have

• High melting points and High boiling points

• Low melting points and High boiling points

• Low melting points and Low boiling points

A large bond dissociation energy corresponds to a

• Weak covalent

• Strong covalent

• Strong ionic

When are two atoms likely to form a double or triple bond

• When they have extra electron pairs

• attain noble gas structure sharing two or three electron pairs

How are atomic and molecular orbitals related?

• 2 atoms combine and have separated orbitals

• atomic orbital belong to a molecule & molecular orbital belong to an atom

• two atoms combine with atomic orbitals overlap to form molecular orbital

VSEPR theory states that molecular shapes adjust to minimize

• attraction between electron pairs.

• hybridization among electron pairs.

• repulsion between electron pairs.

What shape does a sp3 orbital like methane have?

• trigonal planar

• tetrahedral

• linear

More Electronegative atoms in a polar covalent bond gains a partial negative charge

• No

• Yes

What happens when polar molecules are between oppositely charged metal plates?

• Polar molecules have random order

• The molecules stick to one plate more than the other

• The slightly negative ends point to the positive plate

In polar bonds, the more electronegative atom

• attracts electrons and gains a slightly negative charge.

• repels electrons and gains a slightly negative charge.

• attracts electrons and gains a slightly positive charge.