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• Ionic Compounds BaCl2 barium chloride K2O potassium ..., Exercises of Chemistry

Ionic Compounds. – often a metal + nonmetal. – anion (nonmetal), add “ide” to element name. BaCl2 barium chloride. K2O potassium oxide. Mg(OH)2.

Typology: Exercises

2021/2022

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Common Monoatomic Ions
H-hydride
Na+sodium
H+hydrogen
Li+lithium fluoride
F-
Cs+caesium
K+potassium
Ag+silver
chloride
Cl-
bromide
Br-
iodide
I-
Mg2+ magnesium
Sr2+ strontium
Ca2+ calcium
Zn2+ zinc
Ba2+ barium
Cd2+ cadmium
Al3+ aluminium
+1
+2
+3
Cations
Charge Formula Name
Anions
Charge Formula Name
-1
-2
-3
oxide
O2-
sulfide
S2-
nitride
N3-
Ionic Compounds
often a metal + nonmetal
anion (nonmetal), add “ide to element name
BaCl2barium chloride
K2Opotassium oxide
Mg(OH)2magnesium hydroxide
KNO3potassium nitrate
oxoanions often end with ate
pf3
pf4
pf5

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Common Monoatomic Ions

H

  • hydride

Na

sodium

H

hydrogen

Li

lithium fluoride F

Cs

caesium

K

potassium

Ag

silver

chloride Cl

bromide Br

iodide I

Mg

2+ magnesium

Sr

2+ strontium

Ca

2+ calcium

Zn

2+ zinc

Ba

2+ barium

Cd

2+ cadmium

Al

3+ aluminium

Cations

Charge Formula Name

Anions

Charge Formula Name

oxide O

2-

sulfide S

2-

nitride N

3-

  • Ionic Compounds
    • often a metal + nonmetal
    • anion (nonmetal), add “ ide ” to element name

BaCl 2

barium chloride

K 2

O potassium oxide

Mg(OH) 2

magnesium hydroxide

KNO

3

potassium nitrate

oxoanions often end with ate

Some Common Polyatomic Ions

Formula

Cations

NH

4

Common Anions

CH

3

COO

-

H

3

O

Formula

ammonium

hydronium

Name Name

CN

-

acetate

cyanide

OH

- hydroxide

ClO 3

- chlorate

NO

2

- nitrite

NO

3

- nitrate

MnO 4

- permanganate

CO

3

2

-

carbonate

CrO 4

2

-

chromate

Cr 2

O

7

2

-

dichromate

O

2

2

- peroxide

SO

3

2 -

sulfite

PO

4

3 - phosphate

SO

4

2 -

sulfate

e.g. nitrogen forms

2 oxoanions

NO 3

-

NO 2

- “ite”

“ate”

nitrite

nitrate

  • Some elements can form more than 2 oxoanions e.g. chlorine

ClO

- hypochlorite (“ hypo” – least)

ClO 2

- chlorite

ClO 3

- chlorate

ClO 4

- perchlorate (“per” – most)

order as before

  • Anions with hydrogen (add one positive charge i.e addition of H

+ )

e.g. S

**2-

  • H**

+ HS

- hydrogen sulfide

CO 3

**2-

  • H**

+ HCO 3

- hydrogen carbonate

OH

- hydroxide ion

Oxoanions

add “hydrate” preceded by prefix indicating the number of water molecules

e.g. CuSO 4

Cu

2+ , SO 4

2- copper(II) sulfate

CuSO 4

. 5H 2

O

(5 water molecules, called water of hydration)

copper(II) sulfate pentahydrate

1 mono- 2 di- 3 tri- 4 tetra- 5 penta-

6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

Hydrates (compounds that contain water molecules):

Numerical Prefixes for Hydrates and Binary Covalent Compounds

………… often molecular

Molecular compounds

  • nonmetals or nonmetals + metalloids
  • common names H 2

O, NH

3

, CH

4

  • element further left in periodic table is 1

st

  • element closest to bottom of group is 1

st

  • if more than one compound can be formed from the same

elements, use prefixes to indicate number of each kind of

atom

  • last element ends in ide

HI hydrogen iodide

NF

3

nitrogen trifluoride

SO

2

sulfur dioxide

N

2

Cl

4

dinitrogen tetrachloride

Examples:

Guidelines

Sample Problem Naming Binary Ionic Compounds

PROBLEM: Name the ionic compound formed from the following pairs of

elements:

PLAN:

(a) magnesium and nitrogen

SOLUTION:

Use the periodic table to decide which element is the metal and

which the nonmetal. The metal (cation) is named first and we

use the - ide suffix on the nonmetal name root.

(b) iodine and cadmium

(c) strontium and fluorine (d) sulfur and caesium

(a) magnesium nitride

(b) cadmium iodide

(c) strontium fluoride

(d) caesium sulfide