bonding

Question 1

what are the 3 main types of bonding?

Answer 1

covalent, ionic and metallic

Question 2

what types of atom is ionic bonding between?

Answer 2

metal and non metal

Question 3

what is ionic bonding?

Answer 3

the electrostatic force of attraction between oppositely charge ions

Question 4

what structure do ionically bonded compounds form?

Answer 4

giant ionic lattice

Question 5

what is an anion?

Answer 5

a negative ion

Question 6

what is a cation?

Answer 6

a positive ion

Question 7

what two factors affect the strength of ionic bonds?

Answer 7

size of the ions
charge of the ions

Question 8

how does the size of an ion affect the strength of the ionic bond?

Answer 8

the smaller the ion, the stronger the attraction

Question 9

how does the charge of ions affect the strength of the ionic bond?

Answer 9

the greater the charge difference, the stronger the ionic bond

Question 10

what are the properties of ionic compounds?

Answer 10

conduct electricity
high melting point
suluble

Question 11

why do ionic compounds conduct?

Answer 11

if MOLTEN OR DISSOLVED the ions are free to move and carry charge

Question 12

why do ionic compounds have a high melting point?

Answer 12

strong electrostatic forces of attraction need a lot of energy to overcome

Question 13

why are ionic compounds usually soluble in water?

Answer 13

water molecules pull ions away from the lattice causing it to dissolve

Question 14

what type of atoms is covalent bonding between?

Answer 14

non metal + non metal

Question 15

what is covalent bonding?

Answer 15

a shared pair of electrons

Question 16

what is co-ordinate bonding?

Answer 16

when both the electrons come from the same species
the lone pair of electrons on an atom are donated

Question 17

what is the shape of a molecular ion when it has 2 electron pairs?

Answer 17

linear

Question 18

what is the bond angle of a linear molecule?

Answer 18

180

Question 19

what is the shape of a molecular ion when it has 3 electron pairs?

Answer 19

trigonal planar

Question 20

what is the bond angle of a trigonal planar molecule?

Answer 20

120

Question 21

what is the shape of a molecular ion when it has 4 electron pairs?

Answer 21

tetrahedral

Question 22

what is the bond angle of a tetrahedral molecule?

Answer 22

109.5

Question 23

what is the shape of a molecular ion when it has 5 electron pairs?

Answer 23

trigonal bipyramidal

Question 24

what are the bond angles of a trigonal bipyramidal molecule?

Answer 24

90 , 120

Question 25

what is the shape of a molecular ion when it has 6 electron pairs?

Answer 25

octahedral

Question 26

what is the bond angle of an octahedral molecule?

Answer 26

90

Question 27

what is electronegativity?

Answer 27

the power of an atom to attract the electrons in a covalent bond

Question 28

what factors affect electronegativity?

Answer 28

nuclear charge atomic radius shielding

Question 29

how does nuclear charge affect electronegativity?

Answer 29

bigger charge = more attraction

Question 30

how does atomic radius affect electronegativity?

Answer 30

smaller radius = more attraction

Question 31

how does shielding affect electronegativity?

Answer 31

less shells = less shielding = more attraction

Question 32

what are the trends in electronegativity in the periodic table?

Answer 32

increases ACROSS a period increases UP a group

Question 33

why does electronegativity decrease across a group?

Answer 33

- atomic structure increases so more shielding which means less attraction between nucleus and bonding pair

Question 34

why does electronegativity increase across a period?

Answer 34

atomic radius decreases more nuclear charge so stronger attraction

Question 35

what is a polar covalent bond?

Answer 35

covalent bond where the atoms are not shared equally

Question 36

when does a polar bond happen?

Answer 36

when two atoms in a covalent bond have a different electronegativity

Question 37

what are the three types of intermolecular forces?

Answer 37

van der waals permanent dipole dipole hydrogen bonding