Unit 4: ionic bonding

Question 1

cation

Answer 1

a positively charged ion

Question 2

anion

Answer 2

a negatively charged ion

Question 3

swap and drop

Answer 3

a shortcut for determining the ionic compound’s formula: Al⁺³ and O^-2 make Al₂O₃

Question 4

exceptions to swap and drop

Answer 4

sometimes the ratio can be reduced. Ca⁺² and O^-2 don’t make Ca₂O₂; they make CaO

1:1 is a simper ratio than 2:2

Question 5

transition metals

Answer 5

because of the d orbitals, transition metals can have more than one charge.

You need to use a Roman numeral in the name to signify the charge.

Ex: iron III oxide

Question 6

naming ionic compounds

Answer 6

cation name stays the same

anion gets “-ide”

transition metals get a Roman numeral

Ex: mercury II sulfide

Question 7

polyatomic ion

Answer 7

a group of atoms covalently bonded together which together carry a charge.

Question 8

electronegativity difference

Answer 8

Two atoms must have an electronegativity difference of 2 or higher to be considered an ionic compound.

Question 9

periodic chart trend

Answer 9

ionic compounds are always a metal and a nonmetal

the elements come from opposite sides of the periodic chart

Question 10

An alkali earth metal and a halogen will form an ionic compound. What will be the ratio of the elements?

Answer 10

1:2

Ex: CaF₂

Question 11

Elements from group 1 and group 6 form an ionic compound. What will be the ratio of the elements?

Answer 11

2:1

Ex: Na₂S

Question 12

properties of ionic compounds

Answer 12

crystaline, brittle, high melting point, soluble in water

Good conductors of electricity when dissolved in water