Properties of period three elements and their oxides

Which period 3 elements do not combine with oxygen to form an oxide?

chlorine and argon

Oxygen + sodium →

State properties as well

2Na₂O (4Na)
White solid and yellow flame.

Oxygen + magnesium →

State properties as well

2MgO
white solid and white flame

Oxygen + aluminium →

State properties as well

2Al₂O₃
white solid and white flame

What type of oxides are magnesium and sodium oxide?

basic oxides

Which period 3 oxides have giant ionic structures?

sodium

magnesium

aluminium

Why does aluminium foil not readily react with oxygen?

It has a protective oxide layer that prevents reaction. protects aluminium from corrosion

What are basic oxides?

they react with acids

What type of oxide is aluminium oxide?

amphoteric oxide

What is an amphoteric oxide?

has acidic and basic properties

Oxygen + silicone →

State properties as well

SiO₂

White solid

smoke and white flame

giant covalent

What type of oxide is silicon oxide?

acidic

Oxygen + phosphorus →

State properties as well

P₄O₁₀
white solid and white flame

simple covalent

What type of acid is phosphor oxide?

acidic

Why is phosphor oxide stored under water?

prevent contact with air

Oxygen + sulfur →

State properties as well

SO₂
blue flame and choking gas misty fumes

simple covalent

What type of oxide is sulfur dioxide?

acidic

How is SO₃ formed? What type type of oxide is it`?

acidic
Sulfur dioxide is burned in air in the presence of vanadium (V) oxide catalyst.

Equation to form SO₃

2SO₂ + O₂ → 2SO₃

Going across the period what happens to the melting point of the oxides?

decreases

Why are ionic oxides bases? + equation

they contain oxide ion which is a basic ion.

Reacts with water by accepting a proton

O^2- + H₂O _→ 2OH^-

What does the oxide ion behave as?

Bronsted Lowry base

Equation of sodium oxide and water
State pH and the ionic equation

Na₂O(s) + H₂O (l) → 2NaOH (aq)

ph 13/14

Na₂O(s)+ H₂O (l) → 2Na⁺(aq) + 2OH^-(aq)

Sodium oxide + sulfuric acid

And its ionic equation

→ Na₂SO₄(aq) + H₂O(l)

Na₂O (s) + 2H⁺(aq) → 2Na⁺(aq) + H₂O(l)

Sodium oxide + hydrochloric acid

And its ionic equation

→ 2NaCl(aq) + H₂O(l)

Na₂O (s) + 2H⁺(aq) → 2Na⁺(aq) + H₂O(l)

Equation of magnesium and water
State pH and the ionic equation

MgO(s) + H₂O → Mg(OH)₂

ph 9

MgO + H₂O → Mg²⁺ + 2OH^-

Magnesium oxide + Hydrochloric acid

→ MgCl₂ + H₂O

Magnesium oxide + phosphoric acid

3MgO + 2H₃PO₄ → Mg₃(PO₄)₂ + 3H₂O

Magnesium oxide + nitric acid

Ionic equation too

→ Mg(NO₃)₂ + H₂O

MgO + 2H⁺ → Mg²⁺ + H₂O

Describe aluminium oxide reaction with water and state ph

does not react

insoluble in water

ph 7

Why is aluminium oxide insoluble in water?

hydration enthalpy is less than the very high attic enthalpy

Aluminium oxide and hydrochloric acid and the ionic equation

Al₂O₃ + 6HCl -→ 2AlCl₃ + 3H₂O

Al₂O₃ + 6H⁺ → 2Al³⁺ + 3H₂O

Aluminium oxide and sulfuric acid and the ionic equation

Al₂O₃ + 3H₂SO₄ -→ 2Al(SO₄)₃ + 3H₂O

Al₂O₃ + 6H⁺ → 2Al³⁺ + 3H₂O

How does aluminium oxide behave when reacting with sulfuric and hydrochloric acid?

base

Write an equation of aluminium oxide reacting as an acid and the ionic equation

Al₂O₃(s) + 2NaOH(aq) +H₂O(l) → 2NaAl(OH)₄(aq)

Al₂O₃(s) + 2OH^-(aq) + 3H₂O(l) → 2Al(OH)₄^-(aq)

What are all simple covalent molecules?

acidic

Describe reaction of silicon dioxide with water and the ph

ph 7

does not react

insoluble in water

Why is silicon dioxide insoluble in water?

hydration enthalpy is less than bond enthalpy

Equation for silicon dioxide and sodium hydroxide and ionic

SiO₂(s) + 2NaOH → Na₂SiO₃ + H₂O

SiO₂ + 2OH^- → SiO₃^2- + H₂O

Silicon dioxide and potassium hydroxide

SiO₂ + KOH → K₂SiO₃ + H₂O

Silicond dixodie and potassium oxide

SiO₂ + K₂O → K₂SiO₃

Silicon dioxide and magnesium carbonate

SiO₂ + MgCO₃ → MgSiO₃ + CO₂

Phosphor oxide and water

state ph and ionic

P₄O₁₀ + 6H₂O → 4H₃PO₄

ph1

P₄O₁₀ + 6H₂O → 4H+ + 4H₂PO₄^-

Equation and ionic equation of phosphor oxide and sodium hydroxide

P₄O₁₀ + 12NaOH → 4Na₃PO₄ + 6H₂O

P₄O₁₀ + 12OH^- → 4PO₄^3- + 6H₂O

Phosphate and sodium oxide

6Na₂O + P₄O₁₀ → 4Na₃PO₄

Phosphate and magnesium oxide

P₄O₁₀ + 6MgO → 2Mg₃(PO₄)₂

What type off reaction are these:

P₄O₁₀ + 6MgO → 2Mg₃(PO₄)₂

6Na₂O + P₄O₁₀ → 4Na₃PO₄

acid base

Sodium oxide and phosphoric acid

3Na₂O + 2H₃PO₄ → 2Na₃PO₄ + 3H₂O

Reaction of sulfur dioxide and water to form sulfuric (IV) acid

State pH and ionic

SO₂ + H₂O → H₂SO₃

ph3

SO₂ + H₂O → ← H⁺ + HSO₃^-

Reaction of sulfur trioxide and water

State pH and ionic

SO₃ + H₂O → H₂SO₄

ph 0

SO₃ + H₂O → H⁺ + HSO₄^-

Equations for sulfur dioxide and sodium hydroxide

SO₂ + 2NaOH → Na₂SO₃ + H₂O

SO₂ + 2OH^- → SO₃^2- + H₂O

Equations for sulfur trioxide and sodium hydroxide

SO₃ + 2NaOH → Na₂SO₄ + H₂O

SO₃ + 2OH^- → SO₄^2- + H₂O

Sulfur trioxide and magnesium hydroxide

SO₃ + Mg(OH)₂ → MgSO₄ + H₂O

Which oxides have the highest and lowest pH?

high = basic oxides

low = acidic oxides

pg10 questions

s

How do oxyacids form?

When acidic oxides react with water

What are oxyacids?

covalent compounds that form ions in aqueous solutions

Draw structure of phosphoric acid and state the shape and angle

tetra 109.5

Describe structure of phosphoric acid and what type of acid it is

3 hydrogen atoms are acidic as bonded to electronegative O.

triprotic acid

forming 3 different anions as H+ leaves when reacted with bases

Phosphoric acid + sodium hydroxide (2)

→ NaH₂PO₄ + H₂O

3NaOH + H₃PO₄ → Na₃PO₄ + 3H₂O

Shape and bond angles of dihydrogenphosphate ion and hydrogenphosphate(V) ion and phosphate ion (include lone pairs)

H₂PO₄^-
HPO₄^2-

PO₄^3-

all tetrahedral and 109.5

Structure and angle of sulfuric(IV) acid

Sulfuric IV acid and sodium hydroxide

H₂SO₃ + NaOH → NaHSO₃ + H₂O

Sulfuric IV acid and excess sodium hydroxide

H₂SO₃ + 2NaOH → Na₂SO₃ + H₂O

Shape and angle of hydrogensulfate(IV) ion and sulfate(IV) ion

HSO₃^-

SO₃^2-

Trigonal pyramidal 107

Structure and angle for sulfuric acid

Shape and angle of hydrogensulfate(VI) ion and sulfate(VI) ion

HSO₄^-

SO₄^2-

tetrahedral 109.5