Exam 2 notes

Question 1

Ionic compound

Answer 1

held together by the attraction between the positive and negative ions.

Question 2

F-

Answer 2

Floride ion

Question 3

Cl-

Answer 3

cloride ion

Question 4

Br-

Answer 4

bromine ion

Question 5

I

Answer 5

iodide ion

Question 6

O2

Answer 6

oxide ion

Question 7

S2

Answer 7

sulfide ion

Question 8

P3

Answer 8

phosphide ion

Question 9

N3

Answer 9

nitride ion

Question 10

Naming Ions

Answer 10

Add ion (for cation) to the element name.

Ex. Li+ = lithium ion or lithium cation

Question 11

For elements that can form multiple ions

Answer 11

Add the magnitude of the charge to the name

Ex. Fe2+ ion (II) Fe3+(II) Fe1+ (I)

Question 12

Naming ions anions

Answer 12

Add -ide to element name stems.

Ex. Br- = bromide ion
O2 = oxide ion

Question 13

Ionic formula
chem formula for the ionic compound
writing ionic formula

Answer 13

Cation goes 1st; anion goes last
total number of positive charges = total number of negative charges in an uncharged compound.

Ex. LiBr = Li+1 Br-1
NaCl = Na+ Cl-
Mg + O = Mgo
Li+ O2- = Li2O-2
Mg2+ Br1- = MgBr2

Question 14

Naming ionic compounds

Answer 14

1. The cation name goes 1st omit “ion” or “cation.”
2. Anion’s name goes next or last.
   Ex. LiBr2 = Lithium chloride, CaBr2 = Calcium Bromine
3. For cation with more than 1 positive charge.
   Put the charge in (Roman numerals) in parentheses after the cation name.
   Ex. FeCl2
   = iron (II) chloride, FeCl3 = iron (III) chloride,

Question 15

Polyatomic ion

Answer 15

Poly = many
Atomic = atoms
Ion = Charge

Question 15

What she wants us to know:

Answer 15

Ammonium = NH4+
Acetate = C2H3O2- or CH3COO-
Bicarbonate (hydrogen carbonate) = HCO3
Carbonate = CO3^2-
Cyanide = CN-
Hydroxide = OH-
Nitrate = NO3-
Phosphate = PO4^3-
Sulfate = SO3^2-

Question 16

How to find the molar mass formula

Answer 16

Pb3(PO4)
Ex. 1(107.868)= 107.868
2(12.011) = 24.022
2(12.0067) = 28.013
——————————
15.9903

Question 17

Reminder = ionic bonding

Answer 17

Occurs between metals & non-metals

“Thru electrons transfer between atoms forms ions.

Fill outer octet/duet.

Oppositely charged ions attract each other.

Question 18

Electron sharing

Answer 18

Atoms can also fill octets or duets by sharing electrons.

Question 19

Covalent Bond

Answer 19

It occurs when two atoms share electrons to fill outer octets/duets.

Question 20

NaCl

Answer 20

No charge - when they are from different sides/ think ionic.

Bonding pair of electron pairs of electrons involved in a covalent bond.

A molecule group of atoms held together by covalent bonds.

Look in a notebook, for example.

Each hydrogen has two electrons to fill. Its subshell (duet)

Question 21

Single Bond

Answer 21

Covalent bond - consists of two shared electrons (1 pair)

Bonding electron pairs that form a covalent bond

Look in a notebook, for example.

Question 22

It is between two atoms only, but a molecule can have multiple covalent bonds.

Answer 22

Covalent bond

Question 23

Central atoms

Answer 23

atom in the center of a molecule

Question 24

Surrounding atoms

Answer 24

That covalently bonds to the central atoms.

Question 25

How to draw Luis diagrams for molecules (covalent) + ions.

Answer 25

1. Draw Lewis structures of all the atoms
2. Identify the central atom + the surrounding atoms.
3. Add each surrounding atom to the central atom individually.
4. IF THE MOLECULE IS AN ION
   ADD ONE ELECTRON FOR EACH NEGATIVE CHARGE
   REMOVE ONE ELECTRON FOR EACH POSITIVE CHARGE

Look in your notebook for examples.

Question 26

Double Bond

Answer 26

A covalent bond is composed of two pairs of bonding electrons.

Look in a notebook, for example.

Question 27

Triple Bond

Answer 27

A covalent bond is composed of three pairs of bonding electrons.

Covalent typically form between two non-metals. They form by sharing electrons.
Present in polyatomic ions.

Can form ionic bonds between outer charged species.

Look in my notebook for an example.