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Ionic compounds

Ionic compounds

composed of positively and negatively charged ions held together by strong electrostatic forces. Result from the transfer of electrons from one element to another.

Covalent compounds

composed of individual molecules, discrete groups of atoms that share electrons. Result from the sharing of electrons between two atoms

bonding

the process of elements gaining, losing, or sharing electrons to attain the electronic configuration of the noble gas closest to them in the periodic table

types of

ionic bonds are formed between a metal on the left side of the periodic table and a nonmetal on the right side

ions

Charged species in which the number of protons and electrons in an atom is not equal.

cations

positively charged ions. A cation has fewer electrons than protons. Cations are formed by metals.

• for metals in groups 1A, 2A, and 3A, the group number = the charge on the cation

anions

newly updated

Ca²⁺

ion found in teeth and bones

Na⁺ and K⁺

2 ions found in body fluids

Fe²⁺

ion found in hemoglobin

Cl⁻

ion present in gastric juices and other fluids

mg²⁺

ion needed for nerve transmission and muscle control

3 steps to

1. identify which element is the cation and which is the anion (use the group number of a main group element to determine the charge)

2. Determine how many of each ion type is needed for an overall charge of zero.

3. To write the formula, place the cation first and then the anion, and omit charges. (Use subscripts to show the number of each ion needed to have zero overall charge)

2 methods

Systematic Method: follow the name of the cation by a Roman numeral in parentheses to indicate its charge -or- Common Method: Use the suffix -ous for the cation with the smaller charge, and the suffix -ic for the cation with the higher charge. These suffixes are often added to the Latin names of the elements

How to

Replace the ending of the element name by the suffix -ide

3 steps

1. Determine the charge on the cation

2. Name the cation and anion

3. Write the name of the cation first, then the anion

fixed

Al³⁺

Mn²⁺

fixed charge of Mn

Co²⁺

fixed charge of Co

Ni²⁺

Fixed charge of Ni

Zn²⁺

Fixed charge of Zn

Ag⁺

Fixed charge of Ag

Cd²⁺

Fixed charge of Cd

Cr²⁺, Cr³⁺

Variable charges of Cr

Fe²⁺, Fe³⁺

Variable charges of Fe

Cu⁺, Cu²⁺

Variable charges of Cu

Sn²⁺, Sn⁴⁺

Variable charges of Sn

Au⁺, Au³⁺

Variable charges of Au

Pb²⁺, Pb⁴⁺

Variable charges of Pb

3 steps

1. identify the cation and anion and determine their charges

2. Balance the charges of the ions

3. Write the formula with the cation first, and use subscripts to show the number of each ion needed to have zero overall charge

general r

They are extremely high because of the strong electrostatic bonds.

5

• high melting points

• high boiling points

• usually soluble in water

• their solutions conduct electricity

• they form crystalline solids

polyatomic ion

a cation or anion that contains more than one atom

H₃O⁺

formula for hydronium ion

NH₄⁺

formula for ammonium ion

CO₃²⁻

formula for carbonate ion

SO₄²⁻

formula for sulfate ion

PO₄³⁻

formula for phosphate

when to use suffix -ite

used for an anion that has one fewer oxygen atoms than a similar anion named with the -ate ending (ie. SO₄²⁻ is sulfate, but SO₃²⁻ is sulfite)

How to name

the word hydrogen or prefix bi- is added to the name of the anion. (ie. SO₄²⁻ is sulfate, but HSO₄⁻ is hydrogen sulfate or bisulfate)

CO₃²⁻

formula for carbonate

HCO₃⁻

formula for Hydrogen carbonate or bicarbonate

CH₃CO₂⁻

formula for Acetate

⁻CN

formula for Cyanide

NO₃⁻

formula for Nitrate

⁻OHi

formula for hydroxide

SO₄²⁻

formula for Sulfate