Atomic structure + Ionic bonding

Question 1

what elements are involved in ionic bonding?

Answer 1

Metals + non-metals

The element losing an electron becomes a positive ion and the element gaining electrons becomes a negative ion.

Question 2

Common charges of ions

Answer 2

Group 1 always form +1 ions e.g Na+
Group 2 always form +2 ions e.g Mg 2+
Group 6 always form -2 ions e.g O2-
Group 7 always form -1 ions e.g f-

Question 3

Giant ionic substances

Answer 3

• held together by strong electrostatic forces
• high melting and boiling points
• When in solid form do not conduct electricity because their particles are not free to move
  -when molten or dissolved can conduct electricity as the particles can freely move

Question 4

Atomic structure

Answer 4

Protons have a relative mass of 1 and relative positive charge
Neutrons have a relative mass of 1 and 0 relative charge
Electrons have negligible mass and a negative relative charge

Question 5

atomic number

Answer 5

protons/electrons

because they are the same number

Question 6

mass number

Answer 6

protons + neutrons

Question 7

Isotopes

Answer 7

Same protons, different neutrons

because changing protons means changing atomic mass and therefore the element

Question 8

Calculating relative atomic mass (ar)

Answer 8

Ar= total mass of atoms/total number of atoms

example question (doesn’t need to be remembered just for context)-

Calculate the Ar of Pb

Pb- 204=1.4%, Pb-206= 24.1%, Pb- 207 = 22.1% and Pb-208=52.4%

Ar = (204 x 1.4)+(206 x 24.1)+ (207 x 22.1) + (208 x 52.4) / 100 = 207

Question 9

electronic configurations

Answer 9

2,8,8,2

group (vertical) = number of electrons in out shell
row (horizontal) = number of electron shells

Question 10

Hydrogen

Answer 10

(H+).

Question 11

ionic compounds

Answer 11

Are neutral because the protons (+) and neutrons (-) cancel out eachothers charge

Question 12

Electrostatic attraction

Answer 12

The force in between negative and positive ions

Question 13

Group 1 reactivity

Answer 13

Group 1 + water —> Metal hydroxide + Hydrogen

As you go further down group 1 reactivity increases meaning its easier to lose electrons

Question 14

Group 7 reactivity

Answer 14

Reactivity decreases the further you go down group 7 because it has a large atomic radius so there is less attraction of the electrons in the outer shell to the nucleus

Question 15

Group 0

Answer 15

Called Noble gases their outer shell is stable and therefore will not readily react

Question 16

Hydroxide

Answer 16

(OH-)

Question 17

Ammonium

Answer 17

(NH4+).

Question 18

Carbonate

Answer 18

(CO3 2-)

Question 19

Nitrate

Answer 19

(NO3-)

Question 20

Sulfate

Answer 20

(SO4 2-)