Chapter 3: Structure + Properties of Ionic + Covalent Compounds

Question 1

What is a chemical bond?

What electrons are responsible for a chemical bond?

Answer 1

the force of attraction between any two atoms in a compound

valence electrons

Question 2

Ionic vs. Covalent Bonds

Answer 2

Ionic: a transfer of one or more electrons from one atom to another. Octect Rule. Electrons lost by a metal (cation) are gained by a nonmetal (anion)
Covalent: attractive force due to the sharing of electrons between atoms

Question 3

What are the 7 diatomic elements?

Answer 3

diatomic means equal sharing of an element squared

H, N, O, F, Cl, Br, I

Question 4

What is a polar covalent bond?

Answer 4

the bonds are made up of unequally shared electron pairs

Question 5

What is electronegativity?

Answer 5

a measure of the ability of an atom to attract electrons in a chemical bond. higher negativity has a stronger ability to attract electrons. it increases from left to right and bottom to top on the periodic table.

Question 6

Electronegativity Differences

Answer 6

Nonpolar= the sum of electronegativity differences is 0
Polar= 1.9

Question 7

What is a formula?

Answer 7

the representation of the fundamental compound using chemical symbols and numerical subscripts

Question 8

How do you write the names of ionic compounds?

Answer 8

the name of the cation is followed by the name of the anion, which has a suffix of ‘ide’

Question 9

What are the 10 prefixes for naming covalent compounds?

Answer 9

1= mono
2= di
3= tri
4= tetra
5= penta 
6= hexa
7= heat
8= octa
9= nona 
10= deca

Question 10

What prefix is usually omitted from the first element when naming covalent bonds?

Answer 10

mono

Question 11

What suffix is added to the anion when naming covalent bonds?

Answer 11

‘ide’

Question 12

When drawing a lewis structure, the least or most electronegative will be placed in the middle?

Answer 12

least

Question 13

When drawing a polyatomic cation in lewis structure, ________ one electron for every positive charge.

Answer 13

subtract

Question 14

When drawing a polyatomic anion in lewis structure, ________ one electron for every negative charge.

Answer 14

add

Question 15

When drawing a lewis structure, it is important to remember that hydrogen only needs ___ electrons.

Answer 15

2

Question 16

Electrons not involved in bonding are represented as __________.

Answer 16

lone pairs

Question 17

A single bond represents how many electrons?
A double bond?
A triple bond?

Answer 17

2
4
6

Question 18

What does VESPR stand for?

Answer 18

Valence Shell Electron Pair Repulsion: all electrons around the central atom arrange themselves so they can be as far away from each other as possible- to minimize electronic repulsion.

Question 19

According to the VESPR theory; a covalent bond is _______, having specific orientation and an ionic bond has no specific orientation.

Answer 19

directional

Question 20

Molecules that have no lone pair on the central atom and all terminal atoms are the same are ________.

Answer 20

non polar

Question 21

Molecules with one or more lone pairs on the central atom are usually ______.

Answer 21

polar

Question 22

What is the difference between intramolecular and intermolecular forces?

Answer 22

intramolecular forces are attractive forces within the molecule.
intermolecular forces are attractive forces between molecules.

Question 23

Solubility is ____ dissolves _____

Answer 23

like dissolves like