bonding

Question 1

what does the perfect ionic model include

Answer 1

ions are perfectly spherical and the bonding is only ionic with no covalent character

Question 2

what are ionic crystals

Answer 2

ginat lattices of ions when ions are arranged in a regular repeating pattern

Question 3

what is the definition of ionic bonding

Answer 3

the bonding between a metal and non metal resulting in a strong electrostatic attraction between oppositely charged ions in a lattice

Question 4

what are the properties of ionic compounds

Answer 4

high melting points- strong ele. static att. throguhout giant lattice of + and - ions

conduct electricity when molten or dissolved as ions are free to carry a charge

brittle as when ions are moved near a similar charge they allign and repel

soluble in polar solvents as the polarity can aften pull the ions apart and overcome the elec. attraction

Question 5

what is the definition of covalent bonding

Answer 5

when 2 atoms nuclei share a pair or or more of valence electrons

Question 6

what are the properties of giant covalent structures

Answer 6

high melting/ boiling point- multiple strong covalent bonds

rigid- strong covalent bonds

Question 7

what are giant covalent structures and how can carbon form themm

Answer 7

crystal structures with a hige network of covalently bonded atoms which can be formed due to the fact carbon can make 4 covalent bonds

Question 8

what is a dative covalent bond

Answer 8

one atom donated a pair of electrons to from a covalent bond with another atom or ion

Question 9

what is the structure/properties of diamond like

Answer 9

-each c is bonded 4 times

-cannot conduct electricity as no charged particle

-high MP due to many strong covalent bonds

Question 10

what is the structure/properties of silica like

Answer 10

• each Si is bonded to 4 stoms to from lots of covalent bonds

-high MP and BP due to sterong covalent bonds

-doesn’t conduct electricity due to no charged particles

Question 11

what is the structure/properties of graphite

Answer 11

• each carbon forms 3 covalent bonds froming hexagobal rings of carbon atoms arranged in layers

soft and slippery due to layers

high MP due to strong covalent bonds

conducts electricity as the one electron in the outer shell gets released and is a delocalised electron that can caryy a charge

Question 12

what is teh structure/ propoerties of graphine

Answer 12

single layer

extremely strong due to strong covalent bonds

has deloaclised electrons that can carry a charge

Question 13

what is the definition of metallic bonding

Answer 13

strong electrostatic attraction between delocalsied electrons and layers of positive metal ions

Question 14

what are the resulting properties of metallic bonding

Answer 14

malleable- layers of positive metals can slide over each other

high BP/MP- strong electrostatic attraction between delocalised electrons adn + metal ions

good conductors of electricity- delocalised electrons can carry charge freely throughout giant metallic structure

Question 15

what is the bonding in simple molecular compounds and what is the intermolecular force

Answer 15

covalently bonded molecules

multiple molecules held together by weak van der Waals

Question 16

what are the properties of simple moleular substances like

Answer 16

low BP/MP- weak VDW’s meaning little energy to overcome

poor conductors- no charged particles to carry the charge

gases or liwuids at room temp- weak VDW’s

Question 17

what is a molecule and what are they held together by

Answer 17

are 2 or more atoms bonded together held together by covalent bonds

Question 18

what are the 5 common polarised bonds

Answer 18

nitrogen- hydrogen
oxygen- hydrogen
carbon-halogen
carbon-oxygen
hydrogen-halogen

Question 19

when does hydrogen bonding happen

Answer 19

between H and N,O,F

Question 20

hwo does hydrogen bonding work

Answer 20

a lone pair of the electronegative atom N,O or F is attracted to the slightly positively charged H that is bonded to another electronegative atom in a neighbouring molecule

Question 21

how does the permanent dipole intermolecular force work

Answer 21

moleucles with permenant dipoles attract other molecules with permanent dipoles

Question 22

how does the temporary dipole intermolecular force work

Answer 22

movement of electrons can induce a temporary dipole which can induce a temporary dipole in a neighbouring atom so the slightly negative repels the electrons in the neighbouring atom to create a slightly positive charge which attract

Question 23

what is the definition of electronegativity

Answer 23

the ability of an atom to attract the pair of electrons in a covalent bond

Question 24

what factors effect electronegativity

Answer 24

atomic radius- the ability of the nueclus to attract e- dcreases as the atomic radius increases

nuclear charge- the bigger the nuclear charge the higher the ability of the nucleus to attract the e-

electron shielding- the more electron shielding the more repulsion of the electrons so less likely to attract them

Question 25

what does polar mean

Answer 25

an uneven charge distribution

Question 26

what is the definition of an induced dipole

Answer 26

whem the electron orbitals around a molecule are influecnes by another charge

Question 27

what is a permanent dipole

Answer 27

a significant difference in electronegativity causes a permanent polar bond

Question 28

what can multiple polar molecules join together to from

Answer 28

a lattice of molecules

Question 29

each lone pair decreases the bond angle by roughly how much

Answer 29

2.5

Question 30

what is the repulsion trend

Answer 30

lone pair-lone pair repels more than bonded-bonded

Question 31

why are molecules containing polar bonds not always polar overall

Answer 31

if the bonds are symetrical and cancel out the molecule as a whole is non polar

Question 32

why does water bend towards a charged rod

Answer 32

the water molecule has a - and + side to it so the molecule can turn to attract the water and electrostatic attraction is present