Back to marketplace

Period 3

No description yet. This curated deck is ready for daily study.

Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

#1
Front (Question)

Reaction between Na and water, condition observation

Back (Answer)

2Na(s) + 2H20(l) -> 2NaOH(aq) + H2(g) Effervesence Cold water

#2
Front (Question)

What is the product of all of period 3 reacting with oxygen

Back (Answer)

Oxides

#3
Front (Question)

Na + O2 -> ? Flame colour, solid colour

Back (Answer)

4Na(s) + O2(g) -> 2Na2O(s) Yellow flame White solid

#4
Front (Question)

S + O2 -> ? Flame colour, product property

Back (Answer)

S(s) + O2(g) -> SO2(g) Blue flame Choking gas

#5
Front (Question)

Mg, Al, Si and P flame and solid colour

Back (Answer)

White flame White solid

#6
Front (Question)

Mg + O2 -> ?

Back (Answer)

2Mg(s) + O2(g) -> 2MgO(s)

#7
Front (Question)

Al + O2 -> ?

Back (Answer)

4Al(s) + O2(g) -> 2Al2O3(s)

#8
Front (Question)

Si + O2 -> ?

Back (Answer)

Si(g) + O2(g) -> SiO2 (s)

#9
Front (Question)

P + O2 -> ?

Back (Answer)

4P(s) + 5O2(g) -> P4O10(s)

#10
Front (Question)

How are is Na and P stored? Why?

Back (Answer)

Na is under oil. P is under water. To prevent reactions with oxygen.

#11
Front (Question)

Bonding of the metal oxides, examples and properties

Back (Answer)

Ionic Na2O, MgO, Al2O3 Giant ionic lattices, increasing boiling point across the period due to the increasing charge

#12
Front (Question)

Bonding of P4O10 or SO2 oxides and properties

Back (Answer)

Covalent - Simple molecular Weak intermolecular forces, low boiling points, VdW + permanent dipole dipole only

#13
Front (Question)

Why does P4O10 have a larger boiling point then SO2

Back (Answer)

Bigger molecule so more VdW forces

#14
Front (Question)

Bonding of SiO2 oxide and properties

Back (Answer)

Covalent: Macromolecular High boiling point

#15
Front (Question)

Why does Al2O3 show some covalent character

Back (Answer)

Electronegative difference or the small, high charge aluminium ion distorting the oxide charge cloud Less energy to break bonds

#16
Front (Question)

Which are oxides are insoluble to water? Why? pH?

Back (Answer)

Al2O3 due to strong ionic lattice SiO2 due to macromolecular structure pH 7

#17
Front (Question)

Why do metal oxides reacting with water, do they act as a Bronsted-Lowry base or acid? Why?

Back (Answer)

Base Accept protons to form hydroxide ions

#18
Front (Question)

Na2O + H2O -> pH? Colour?

Back (Answer)

Na2O(s) + H2O(l) -> 2Na+(aq) + 2OH-(aq) pH 13 Colourless solution

#19
Front (Question)

MgO + H2O -> pH and why?

Back (Answer)

MgO(s) + H2O(l) -> Mg(OH)2(s) pH 9 Sparingly soluble so only some OH ions are made

#20
Front (Question)

P4O10 + H2O -> pH? Colour? Equation?

Back (Answer)

P4O10(s) + H2O(l) -> 4H3PO4(aq) pH 0 Colourless solution H3PO4 -> 3H+ + PO42-

#21
Front (Question)

SO2 + H2O -> pH? Solution reaction?

Back (Answer)

SO2(g) + H2O(l) -> H2SO3(aq) pH 3 SO2 + H2O -> H+ + HSO3-

#22
Front (Question)

SO3 + H2O -> pH? Solution reaction?

Back (Answer)

SO3(g) + H2O(l) -> H2SO4(aq) pH 0 SO3 + H2O -> H+ + HSO4-

#23
Front (Question)

General equation for when an acid and base react

Back (Answer)

Acid(s) + Base(aq) -> Salt(aq) + water(l)

#24
Front (Question)

What does it mean that Al2O3 is amphoteric?

Back (Answer)

Acts as both an acid and an alkili so can react with both