ionic bonding (checklist)

Question 1

an ion is

Answer 1

an electrically charged atom or group of atoms formed by the loss or gain of electrons

Question 2

why do ions need to lose or gain electrons

Answer 2

to obtain a full outer shell of electrons

Question 3

Negative ions are called

Answer 3

anions

Question 4

anions form when

Answer 4

atoms gain electrons, meaning they have more electrons than protons

Question 5

positive ions are called

Answer 5

cations

Question 6

cations form when

Answer 6

atoms lose electrons, meaning they have more protons than electrons

Question 7

all metals lose or gain electrons to become positively charged ions ?

Answer 7

lose

Question 8

all non metals ____ electrons to become negatively chraged ions

Answer 8

gain

Question 9

Elements in Group 1 form ions with a ___charge

Answer 9

1+

Question 10

Elements in Group 2 form ions with a ___charge

Answer 10

2+

Question 11

Elements in Group 6 form ions with a ___ charge

Answer 11

2-

Question 12

silver is

Answer 12

Ag +

Question 13

copper is

Answer 13

Cu2+

Question 14

iron is

Answer 14

Fe 2+

Question 15

Lead is

Answer 15

Fe2+

Question 16

Zinc

Answer 16

Zn2+

Question 17

Hydrogen

Answer 17

H+

Question 18

Ammonium

Answer 18

NH4+

Question 19

Hydroxide

Answer 19

OH-

Question 20

Nitrate

Answer 20

NO3-

Question 21

Carbonate

Answer 21

CO₃²+

Question 22

Sulfate

Answer 22

SO₄²-

Question 23

what is an ionic bond in terms of electrostatic attractions

Answer 23

electrostatic attraction between oppositely charged ions

Question 24

ionic compounds form

Answer 24

giant ionic lattices

Question 25

giant ionic lattices are made up of

Answer 25

many oppositely charged ions held together by strong electrostatic attractions

Question 25

why do giant ionic lattices have a high melting and boiling point

Answer 25

because it takes a lot of energy to break the electrostatic attraction, or the bonds holding them together

Question 26

why do solid ionic compounds not conduct electricity

Answer 26

because there are no free electrons or ions that can move so cannot conduct electricity

Question 27

when can ionic compounds conduct electricity

Answer 27

when molten or in an aqueous solution

Question 28

why can giant ionic lattices conduct electricity when molten

Answer 28

because the ions are free to move and so can carry charge

Question 29

The lattices formed by ionic compounds

Answer 29

consist of a regular arrangement of alternating positive and negative ions

Question 30

Ionic compounds are poor conductors in the solid state because (2)

Answer 30

The ions are in fixed positions in the lattice They are therefore unable to move and carry a charge

Question 31

Ionic compounds are good conductors of electricity in the molten state or in solution because

Answer 31

When the ionic compound is melted or dissolved in water, the ions are able to move and carry a charge

Question 32

simple molecular structures have low melting and boiling points because

Answer 32

the weak intermolecular forces are easily overcome and take only a small amount of energy to break.

Question 33

As the relative molecular mass of a simple molecular structure increases so does the melting point/boiling point because

Answer 33

The weak intermolecular forces are stronger in larger molecules because they have more electrons.

Question 34

a giant covalent structure is a ( state) and has ___ melting and boiling point

Answer 34

solid high

Question 35

most covalently bonded substances form

Answer 35

simple molecular structures

Question 36

when you melt or boil giant covalent structures, what need to be broken

Answer 36

the strong covalent bonds

Question 37

properties of diamond (3)

Answer 37

- very hard (made of strong covalent bonds so hard) - cannot conduct electricity because there are no free electrons - high melting and boiling point

Question 38

properties of graphite

Answer 38

- high melting and boiling point as it has layers of carbon atoms covalently bonded together - weak intermolecular forces between the layers so the layers can move past each other making it soft and slippery - has a sea of delocalised electrons so can conduct electricity

Question 39

is diamond a giant covLENT STRUCTURE

Answer 39

yes

Question 40

is C60Fullerene a giant covalent structure

Answer 40

yes

Question 41

properties of c60fullerene

Answer 41

- low melting and boiling point because there are weak intermolecular forces between each molecule. - This also makes it soft. - It has delocalised electrons that are free to move around the structure so can conduct electricity

Question 42

do giant covalent structures usually conduct electricity

Answer 42

no