Simple Ions

Front 1

Why does Oxygen (O) react with magnesium(Mg) and not with Neon( Ne)?

Back 1

Oxygen – ( 8 ) ( 2, 6 ) needs to gain 2 electrons to be stable.
Magnesium ( 12) ( 2, 8 , 2) needs to remove 2 electrons to be stable.
Neon ( 10 ) ( 2, 8 ) already has 8 electrons and is stable.
Mg + O2  Mg2O

Front 2

How can you determine how many electrons are in the outermost shell of an atom?

Back 2

-

Front 3

Why are noble gases the least reactive Elements?

Back 3

Noble gases have the greatest number of electrons possible in their V.E making them stable & less reactive

Front 4

Octet rule

Back 4

Atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electronic configuration as a noble gas.
Eg. CO2
C- ( 6) 2, 4
O (8 ) 2, 6

Back 5

An atom that has gained or lost electrons and has a negative / positive charge.
Na+
Cl -

Back 6

Alkali metals ( Group 1 ) has 1 electron in V.E and can give it away to be stable.
Halogens ( Group 17 ) needs 1 electron to be stable

Back 7

K (19)
Electron configuration same as _____-

Back 8

Cl(17)
Electron configuration same as _____

Back 9

Ions have an electrical charge so it forms compounds.
Conducts electricity when dissolved in water.

Front 10

Atoms & ions

Back 10

When atoms form ions they do not actually become noble gases. They only have identical electronic configuration.
Na(11) –
Na+ (10) –

Back 11

Na- extremely reactive with H2O
Cl – poisonous yellow green gas.
Na+ Cl NaCl
Formed from 2 dangerous elements , but it is consumable as table salt.
This is because the ions have different electron configuration & charge as compared to the parent atoms.

Front 12

Metals form cations

Back 12

Mg ( 12)
Electronic configuration – 2, 8 , 2
Mg – 2 e- Mg 2+
2, 8 , 2 2, 8
Mg ion is stable as it contains 8 electrons in the V.E

Back 13

O ( 6) 2, 6
O +2e  O 2- (2, 8 )
O 2- has the same configuration as Neon ( Ne)

Back 14

Q 10 & 11 in your copy book.