Ionic Bonding GCSE flashcards

what type of ions do metals form

positive cations- lose electrons from outermost shell

what type of ions do non metals form

negative anions- gain electrons into their outermost shell

what determines the size of charge on the ion

the group the element is in

group 1 atoms lose 1 electron from their outermost shell to from an ion with a … charge

1+

group 2 atoms lose 2 electrons from their outermost shell to from an ion with a … charge

2+

state the ionic formula of lithium

Li⁺

group 6 atoms gain 2 electrons into their outermost shell to form an ion with a …charge

2-

name the ionic formula of an oxide ion

(O)²⁻

state the ionic formula for the metals:

1. ammonium

2. magnesium

3. iron (III)

1. (NH4)⁺

2. (Mg)²⁺

3. (Fe)³⁺

state the ionic formula for the non metals:

1. chloride

2. hydroxide

3. nitrate

4. oxide

5. sulfate

6. sulfite

7. carbonate

8. nitride

9. phosphate

1. Cl⁻

2. OH⁻

3. (NO₃)⁻

4. (O)²⁻

5. (SO₄)²⁻

6. (SO₃)²⁻

7. (CO₃)²⁻

8. (N)³⁻

9. (PO₄)³⁻

how to find the formula for the ionic compound lithium fluoride

1. Li⁺ and F⁻

2. both have charge of 1+ or 1-

3. so no more ions need to be added because charges cancel each other out

4. formula: LiF

how to find the formula fro the ionic compound magnesium hydroxide

1. Mg²⁺ and OH⁻

2. charges don’t cancel, so another OH⁻ ion needs to be added

3. so formula: Mg(OH)₂

state the ionic compound formula for the ions

1. Na⁺ and F⁻

2. Mg²⁺ and O²⁻

3. Cu²⁺ and Br⁻

4. Na⁺ and (CO₃)²⁻

5. (NH₄)⁺ and (SO₄)²⁻

6. Fe³⁺ and O²⁻

7. Al³⁺ and (CO₃)²⁻

1. NaF

2. MgO

3. CuBr₂

4. Na₂CO₃

5. (NH₄)₂SO₄

6. Fe₂O₃

7. Al₂(CO₃)₃

the overall charge on an ionic compound must be…

ZERO

how can you tell whether a compound is ionic or not

metal + non metal = ionic

describe the formation of the ionic compound Lithium Fluoride by electron transfer

1. Lithium- 2,1

2. Fluorine- 2,7

3. one lithium atom loses one elecron to became an Li⁺ cation [2]⁺

4. one fluorine atom gains this electron from the lithium atom to become F⁻ anion [2,8]⁻

5. Li⁺ and F⁻ both attract each other with an electrostatic force of attraction

6. forming the ionic lattice structure lithium fluoride

describe the formation of the ionic compound Calcium Chloride by electron transfer

1. Chlorine- 2,8,7

2. Calcium- 2,8,8,2

3. one calcium atom loses 2 electrons to become Ca²⁺ cation [2,8,8]²⁺

4. two chlorine atoms each gain 1 electron from the Ca atom to become Cl⁻ anions [2,8,8]⁻

5. Ca²⁺ and 2 x Cl⁻ attract each other with electrostatic forces of attraction

6. forming ionic lattice structure CaCl₂

do ionic compounds conduct electricity when in a solid state and why

no- the ions are not free to move and are in fixed positions in the lattice, so there is no flow of charge throughout the structure

why do ionic compounds have no overall charge

the charges on the ions cancel each other out

where do the electrostatic forces of attraction occur in ionic bonding

between oppositely charges ions, acting in all directions, very strong

in which states do ionic compounds conduct electricity

molten or aqueous solution

why can ions conduct electricity when molten or in aqueous solution

ions are free to move, so their is a flow of charged particles throughout the structure

are electrostatic forces of attraction strong or weak

strong- so lots of energy is needed to overcome them

explain why potassium fluoride has a very high melting point

• ionic lattice structure

• with strong electrostatic forces of attraction

• between oppositely charges ions

• that need a lot of energy to overcome them

complete pages 37, 38, 39

okay