Test 3 Definitions

Question 1

Ionic Bonds

Answer 1

Ionic bonds occur when the atoms of one element lose valence electrons, while another element gains valence electrons. (Transfer of valence electrons drawn by electrostatic attraction)

Question 2

Covalent Bonds

Answer 2

Covalent bonds occur when non-metal atoms share electrons to attain a noble gas arrangement. (Sharing of electrons)

Question 3

Octet Rule

Answer 3

Stable ions and stable atoms in a bond have a full outer shell; this means for row 2 and on, atoms/ions need access to 8 electrons. Exception: Hydrogen needs access to 2

Question 4

Shapes of Molecules: What does molecular geometry include?

Answer 4

Lone pairs need space, just as bonds do. Molecular geometry only includes the atoms and the bonds.

Question 5

Shapes of molecules: 2 pairs, 0 Lone

Answer 5

Linear

Question 6

Shapes of molecules: 3 pairs, 0 lone

Answer 6

Trigonal Planar

Question 7

Shapes of molecules: 2 pairs, 1 lone

Answer 7

Bent

Question 8

Shapes of molecules: 4 pairs, 0 lone

Answer 8

Tetrahedral

Question 9

Shapes of molecules: 3 pairs, 1 lone

Answer 9

Trigonal Pyramidal

Question 10

Shapes of molecules: 2 pairs, 2 lone

Answer 10

Bent

Question 11

Polar Bonds

Answer 11

Polar bonds are formed when two atoms share a pair of electrons (covalent bond), but one of the two atoms has a greater attraction for electrons. They are more likely to be found closer to that nucleus. Which now has a higher density.

Question 12

Electronegativity > 1.8

Answer 12

Ionic

Question 13

Electronegativity < 0.5

Answer 13

Non-polar

Question 14

Electronegativity <= 0.5 - >= 1.8

Answer 14

Polar

Question 15

Electronegativity

Answer 15

measures the tendency of an atom to attract a bonding pair of electrons (based on experimental data)

Question 16

Dipole-Dipole Attractions

Answer 16

Polar Molecules. The partial positive part of one molecule is attracted to the partial negative part of a neighbor.

Question 17

What is the direction of polarity?

Answer 17

Positive to Negative

Question 18

When is hydrogen bonding possible?

Answer 18

When hydrogen is bonded to Nitrogen, Oxygen, or Fluorine

Question 19

Can Acetone bond with itself? O = C – CH3 – CH3

Answer 19

No. There is hydrogen on carbon, but not on Nitrogen, oxygen, or fluorine

Question 20

Order of increasing force: Hydrogen bonding, covalent bonds, dispersion forces, and dipole-dipole forces

Answer 20

(Lowest Force) Dispersion Forces, Dipole- Dipole, Hydrogen Bonding, Covalent Bonds (Highest Force)

Question 21

What are 4 effects of water having hydrogen bonding?

Answer 21

A high melting point, a large liquid range, a very high boiling point, and surface tension (helps dissolve) ALSO, ice floats

Question 22

Effects of intermolecular attraction?

Answer 22

• Stronger molecular forces bring molecules together, creating a condensed phase like liquid or solid (molecules have to overcome intermolecular interactions to transition between solid, liquid, and gas)
• Stronger intermolecular forces demand more energy (heat) to transition from solid, liquid, and gas).
• In liquids, molecular attractions cause viscosity and surface tension