bonding

Question 1

ionic compounds contain..

Answer 1

a metal and non metal

Question 2

what happens when ionic compounds form

Answer 2

electron transfer

Question 3

what us a single covalent bond

Answer 3

a shared pair of electrons

Question 4

what does the number of unpaired electrons indicate?

Answer 4

the number of covalent bonds that can be made

Question 5

how many covalent bonds can carbon make

Answer 5

4

Question 6

what is an ion?

Answer 6

a charged particle

Question 7

what are cations?

Answer 7

positive ions

Question 8

what are anions?

Answer 8

negative ions

Question 9

what is an ionic bond?

Answer 9

the elctrostatic attraction between oppositely charged ions

Question 10

what do elements lose/gain electrons to achieve?

Answer 10

nobel gas configuration

Question 11

what is different about transition metals?

Answer 11

do not always achieve nobel gas configuration

Question 12

what is an ionic lattice?

Answer 12

regular, repeated 3D framework of ions

Question 13

what is each:

1) Na+ ion sureounded by in NaCl

2) Cl- ion sureounded by in NaCl

Answer 13

1) 6 Cl- ions

2) 6 Na+ ions

Question 14

what tyoe of crystal structure is NaCl?

Answer 14

cubic

Question 15

what is decrepitation?

Answer 15

cracking sounds made when an ionic crystalline structure breaks up upon heating

Question 16

why does ionic solids have high melting points?

Answer 16

strong electrostatic attractions between oppositely charged ions require alot of energy to break

Question 17

what increases the strength of ionic bonds?

Answer 17

smaller ions and higher charge

Question 18

why are positive ions smaller than their atoms

Answer 18

losing an electron from an outer shell inscreases the effective nuclear charge pulling electrons closer to the nucleus

Question 19

why are negative ions larger than their atoms?

Answer 19

effective nuclear charge decreases and increases electron repulsion

Question 20

wht are ionic compounds usually soluble in water?

Answer 20

water is a polar solvent

Question 21

why are some ionic compounds not soluble in water

Answer 21

the electrostatic attraction is so strong, water cannot break the lattice apart

Question 22

why can ionic compounds conduct electrocity when molten or dissolved?

Answer 22

charges are free to move and transport a current

Question 23

how is a single covalent bond represented

Answer 23

a line

Question 24

how is a double covalent bond represented

Answer 24

a double line

Question 25

what is a lone pair

Answer 25

a pair of electrons not involved in bonding

Question 26

whoch orbitals are used if bonding results in more than 8 calence electrons?

Answer 26

d orbitals

Question 27

what is another name for a dative covalent bond

Answer 27

coordinate bond

Question 28

what is a dative covalent bond?

Answer 28

a lone pair is donated into an empty orbital on another atom

Question 29

what is different about a dative covalent bond?

Answer 29

both electrons come from one atom

Question 30

how do you represent a dative covalent bond?

Answer 30

an arrow

Question 31

what is different about the properties of a dative covalent bond and a standard covalent bond?

Answer 31

nothing

Question 32

define metallic bonding

Answer 32

electrostatic forces between delocalised electrons and positive metal ions in a lattice

Question 33

why can metals conduct electricity?

Answer 33

delocalised electrons can transport a current

Question 34

why can metals conduct heat?

Answer 34

delocalised electrons can transfer energy

Question 35

why are metals malleable/ductile?

Answer 35

laters of metal ions can slide over eachother without distrupting the bonding

Question 36

why do metals have high boiling points?

Answer 36

requires a lot of energy to break strong electrostatic atteaction between delocalised electrons and positive metal ions

Question 37

why do transition metals have higher boiling points?

Answer 37

large number of d subshell, electrons delocalise forming stronger bonds

Question 38

what is another name for a giant covalent structure?

Answer 38

macromolecular

Question 39

what are crystal structures of simple covalent compounds called?

Answer 39

molecular covalent crystals

Question 40

give an example of a molecular covalent crystal

Answer 40

ice

Question 41

name three properties of molecular covalent crystals:

Answer 41

low melting point brittle do not conduct electricity

Question 42

what is an allotrope?

Answer 42

different forms of the same element in the same physicao state

Question 43

give two allotropes of carbon

Answer 43

diamond graphite (graphene)

Question 44

give three properties of diamond

Answer 44

hard high melting point does not conduct electricity

Question 45

give three properties of graphite

Answer 45

lubricant high melting point does conduct electricity

Question 46

what is sublimination?

Answer 46

change of state from solid to gas

Question 47

why do lone pairs cause more repulsion?

Answer 47

held closer to the nucleus

Question 48

2 bonding pairs 0 lone pairs: name angle

Answer 48

linear 180•

Question 49

3 bonding pairs 0 lone pairs: name angle

Answer 49

trigonal planar 120•

Question 50

4 bonding pairs 0 lone pairs: name angle

Answer 50

tetrahederal 109.5•

Question 51

3 bonding pairs 1 lone pair: name angle

Answer 51

pyramidal 107•

Question 52

2 bonding pairs 2 lone pairs: name angle

Answer 52

bent 104.5•

Question 53

5 bonding pairs 0 lone pairs: name angles

Answer 53

trigonal bypyramid 90• and 120•

Question 54

3 bonding pairs 2 lone pairs: name angle

Answer 54

T shaped 86•

Question 55

2 bonding pairs 3 lone pairs: name

Answer 55

linear

Question 56

6 bonding pairs 0 lone pairs: name angle

Answer 56

octahederal 90•

Question 57

4 bonding pairs 2 lone pairs: name angle

Answer 57

square planar 90•

Question 58

4 bonding pairs 1 lone pair: name angles

Answer 58

sawhorse 86• and 117•

Question 59

what is electronegativity?

Answer 59

the power of an atom to attract electron density towards itself

Question 60

wht is the most electronegative element?

Answer 60

fluorine

Question 61

what does electronegativity depend on?

Answer 61

atomic radius- smaller=stronger attraction nuclear charge- more protons=stronger attraction shielding- more e-=more shielding=less attraction

Question 62

what is the trend in electronegativity?

Answer 62

increases across a period and up a group /^

Question 63

what dies a delta +ve charge represent?

Answer 63

electron efficient

Question 64

what does a delta -ve charge represent?

Answer 64

electron rich

Question 65

why is BF3 non-polar

Answer 65

it is symmetrical

Question 66

what is another word for polar?

Answer 66

permenant dipole moment

Question 67

what is an intermolecular force?

Answer 67

a force between molecules

Question 68

what is an intramolecular force?

Answer 68

a force within molecules

Question 69

name theee types if intermolecular force

Answer 69

Van dee Waal dipole-dipole Hydrogen bond

Question 70

how do VDW forces occur?

Answer 70

random movement of electrons causes a temporary dipole which induces a dipole in a neighbouring atom, the resulting opposite delta charges attract

Question 71

what are teo other names for VDW forces?

Answer 71

induced dipole-dipole london forces

Question 72

what happens to VDW attraction as atomic radius increases

Answer 72

gets stronger

Question 73

what is a permenant dipole-dipole force?

Answer 73

interaction between teo permenant dipoles due to the attraction of opposite delta charges

Question 74

which theee bonds can form hydrogen bonds?

Answer 74

N-H O-H F-H

Question 75

which intermolecular force is the strongest?

Answer 75

hydrogen bonds

Question 76

why is ice less dense than water?

Answer 76

hudrogen bonds form an open crystalline structure

Question 77

what sort of molecules dissolve in polar solvents?

Answer 77

polar molecules

Question 78

what sort if molecules dissolve in non-polar solvents?

Answer 78

non-polar molecules