Chemistry Unit 5 Content Quiz Naming compounds and Writing Formulas

Metals tend to _____ ?

Lose e-

Metals form ______ after losing e-?

Cations

Cations

Positviely charged ions, when neautral atom loses 1 or more e-, causing there to be more p+ than e-

Nonmetals tend to _____?

Gain e-

Nonmetals tend to form _____?

Anions

Anions

Negatively charged ions, formed when atoms gains 1 or more e-

The sum of charges in ionic compounds must be____?

Zero overall, ( + balance - )

Formula unit

smallest whole # repeating ration of an ionic coumpund, resulting in neatural charge

Binary Ionic compounds

Binary = 2, Metal + Nonmetal

Steps for writing the formula for an ionic compound

1. identify cation and anion

2. determine charge

3. detemine how many of each are neede for a zero overall charge

(if cation and anion have diff charges, ion charges determine # of each)

Main group cation

Groups 1, 2, 13
Metal + ion
ex: Lithium → Lithium ion

Naming anions

Nonmetal stem + “-ide” + “ion”
ex: Bromine → Bromide ion

Naming Binary Ionic compounds

Cation + anion
Metal Nometal + “-ide”

ex: NaF → sodium fluoride

Ionic charge of transition metal

Roman numeral
or
“-ous” added to root Metal w/ lower ion charge
“-ic” added to root Metal w/ higher ion charge
ex: FeCl2 → Ferrous Chloride

Polyatomic ion w/ (+) ion present

1. Polyatmoic ion name

2. stem of nonmetal

3. suffix “-ide”

ex: Nh4Cl → Ammonium ChloridePo

Polyatmoic ion w/ (-) ion present 

1. Full metal name

2. possible roman numeral

3. Polyatomic ion name

ex: Ca(Mno4)2 → Calcium permanganate

Polyatmoic ions w/ both ions polyatmoic

1. (+) Polyatomic name

2. (-) Polyatmoic name

ex: NH4NO3 → Ammonium nitrateN

Naming ionic compounds forming 1 (+) ion—Metal or ammonium

Use name of element of ammonium

Naming ionic compounds forming more than 1 (+) ion—Metal or ammonium

Use element name + Roman numeral charge

Naming ionic compounds forming single (-) ion—Nonmetal

Use element + “-ide”

Naming ionic compounds w/ polyatmoic atom—Nonmetal

Polyatomic ion name

Naming Covalent compunds

Greek prefixes, 1st nonmetal by element name, 2nd w/ suffix “-ide”
ex: P2O5 → diphosphorus pentaoxide

Ionic vs. Covalent bonding

Ionic:

1. Transfer of e-

2. nonmetal + metal

3. formula units

4. empirical formula

Covalent:

1. sharing of e0

2. 2 nonmetals

3. molecular formula

Emprical formula 

lowest whole # ratio

Molecular formula

represents the actual # of atoms of each element in a molecule of a compound

Mono

1

Di

2

Tri

3

Tetra

4

Penta

5

Hexa

6

Hepta

7

Octa

8

Nona

9

Deca

10

Acid

a substance that produces Hydrogen ions dissolved in water

Naming binary acid

“hydro + nonmetal root + ”-ic” acid
-add as much H to cancel out the charge
(HX)

Naming Oxyacid

Acid of anions;

-name based on polyatomic ions

-ate → “-ic” acid
-ite → “-ous” acid

HXOL

Hydrate

An ionic compound w/ a specific # of water molecules within its solid lattice structure
ex: BaCl₂ ∙ 2H₂O

Naming a hydrate

Name the ionic compound followed by a Greek prefix indicating the number of water molecules and the word “hydrate”
ex: CuSO₄ ∙ 5H₂O → Copper(II) sulfate pentahydrate

Polyatomic rules 1 less O

end in “-ite”

Polyatomic rules 2 less O

end in “-ite”, prefix hypo

Polyatomic rules 1 more O

end in “-ate”, prefix per

Polyatomic rules Hydrogen attached

prefix Hydrogen or bi

binary molecular compounds

2 nonmetals are held together by covalent bonds NOT ionic bonds.

Rules for Naming Type III Binary molecular Compounds:

1st full name element in the formula is named, 2nd element is named as though it were an anion.

Ex: CO2 → carbon dioxide
Drop the ending of oxygen and add the suffix “ide”.
Oxygen becomes oxide.

Polyatmoic ion

group of atoms covalently bonded that has an overall charge (too few or too many electrons) and behaves like a single ion in ionic compounds.

Binary acid

H + monoatomic anion (no oxygen).

oxyacids

H + polyatomic oxoanion (contains oxygen