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chemistry > 1.3 Bonding > Flashcards

1.3 Bonding Flashcards

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1
Q

Nickel is a metal with a high melting point. Explain why it has a high melting point in terms of structure and bonding

A

Structure is giant metallic lattice
Bond is metallic bonding
Where there is strong electrostatic forces between positive metal ions and delocalised electrons

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2
Q

Nickel is a meal. Explain why Nickel is ductile

A

Metals are malleable as layers can slide over each other

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3
Q

Why does calcium have a higher melting point than methane

A

Calcium has a metallic lattice and strong metallic bonding
Methane has a simple molecular structure and weak intermolecular forces between molecules
Metallic bonding in Calcium is stronger than the IMF between CH4
More energy needed to overcome metallic bonds in Calcium

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4
Q

In terms of structure and bonding explain why Sodium oxide has a higher melting point than phosphorus pentoxide (P4010)

A

Sodium oxide has an ionic lattice with ionic bonding
P4O10 has simple molecular structure with intermolecular forces between molecules
Ionic bonding in Sodium oxide is greater than the IMF in P4010

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5
Q

In terms of structure and bonding why does diamond have a higher melting point than strontium

A

Diamond has a macromolecular structure with covalent bonds between atoms
Strontium has a metallic lattice and metallic bonding
Covalent bonding is stronger than metallic bonding
More energy is needed to overcome the covalent bonds in diamond.

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6
Q

Explain why aluminium has a higher melting point than magnesium

A

Aluminium has more protons and has a higher charge
Attracts delocalised electrons more slowly
Forming stronger metallic bonds

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7
Q

Deduce type of crystal shown by graphane

A

Marcomolecule

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8
Q

State how two carbon atoms form a carbon-carbon bond in graphane

A

Shared pair of electrons
One electron from each Carbon atom

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9
Q

Deduce emipircal formula of graphane

A

CH

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10
Q

Two physical properties of silicon dioxide

A

Hard /
Brittle /
Insoluble /
Non conductor

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11
Q

State structure of solid phosphorus oxide

A

Macromoleular

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12
Q

Why does diamond and graphite have high melting points

A

They have many strong covalent bonds in a gaint ionic lattice

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13
Q

Why is graphite a good conductor of electricity

A

There are free movng electrons that can carry a current

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14
Q

Why is graphite soft

A

It has weak intermolecular forces between layers

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15
Q

Explain why melting point of sodium chloride is high

A

Strong electrostatic attraction between oppositely charged ions
Lots of energy required to break

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16
Q

Compare electrical conductivity of solid sodium metal with that of solid sodium chloride

A

Sodium chloride cant and sodium metal can because it has free delocalised electrons that flow through the metal allowing electrons to carry a current.
Ions cant move in a solid salt

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17
Q

Suggest why melting point of sodium iodide is lower than that of sodium bromide

A

Ionic bonds in NaI are weaker because Iodide ion is bigger than a bromide ion so it has a weaker attraction to the Na^+ ion

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18
Q

Type of crystal structure in zinc fluoride

A

Giant ionic lattice

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19
Q

State type of bonding in silver

A

Metallic bonding

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20
Q

What is the name of this bond N-> H
Explain why an arrow is used

A

Dative covalent bond
Lone pair of electrons are donated to hydrogen from nitrogen

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21
Q

NHF2 reacts with BF3
State type of bond formed between N atom and the B atom in F2HNBF3

A

Dative covalent bond
Lone pair of electrons from N atom donated to B atom

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22
Q

Name of shape and bond angle in BF3

A

Trigonal planar
120

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23
Q

Name of shape and bond angle in CCl2

A

2 bp
1 lp
V - shaped
117.5

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24
Q

Shape name of CH4 and bond angle

A

4bp
Tetrahedral
109.5

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25
Q

Shape name and bond angle of NH3

A

3 bp
1lp
Pyramidal
107

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26
Q

Shape name and bond angle of H2O

A

2 lp
2 bp
V - shaped
104.5

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27
Q

Shape name and bond angle of PCl5

A

Trigonal bipyramidal
5 bp
90 and 120

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28
Q

Shape name and bond angle of SF4

A

4 bp
1lp
89 and 119
Seesaw

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29
Q

Shape name and bond angle of ICl3

A

Trigonal planar
3 bp
2 lp
120

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30
Q

Shape name and bond angle of SF6

A

6 Bp
Octahedral
90

31
Q

Shape and bond angle of IF5

A

Square pyramidal
5 bp
1 lp
89

32
Q

Shape and bond angle of XeF4

A

4 bp
2 lp
Square planar
90

33
Q

Shape of TIBr5^2-

A

5bp
trigonal bypramidal

34
Q

Shape name and bond angle of ClF2^-

A

2 bp
3 Lp
Linear
180

35
Q

Explain how electron pair repulsion theory can be used to deduce the shape of, and the bond angle in NHF2 (6)

A

N has 5 electrons in its outer shell
With 2 electrons from F and 1 electron from H, it has a total of 8 electrons in its outer shell
This gives 3 bonding pairs and 1 lone pair
Electron pairs repel as far as possible
Lone pairs repel more than bonding pairs
Therefore it has a pyramidal shape
With angle of 109.5 decreased to 107

36
Q

Explain why CF4 has a bond angle of 109.5 degrees

A

It has a tetrahedral shape and 4 bonding pairs and no lone pairs. Therefore these repel equally

37
Q

State and explain bond angle in H2O

A

2Lp and 2bp so 104.5
Lone pairs repel more strongly than bond pairs so bond angle is reduced from 109.5 degrees to 104.5

38
Q

SCL2 reacts with NaF to form SF4 and S2CL2 and one other product. Write equation for this reaction

A

Product formed NaCl
3SCL2 + 4NaF -> SF4 + S2CL2 + 4NaCl

39
Q

In a POCl3 molecule the oxygen atom is attached to the phosphorus atom by a double bond. Name shape

A

Distorted tetrahedral

40
Q

NH3 + AlCL3 -> H3NAlCl3
Name type of bond formed between N and Al in product formed and explain how it is formed
Explain how value of Cl-Al-Cl bond angle in AlCl3 changes on formation of H3NAlCl3

A

dative covalent bond
Lone pair of electrons from N donated to Al
Aluminium is now surrounded by 4 electrons and shape is tetrahedral therefore bond angle decreases from 120 degrees to 109.5 degrees

41
Q

Define term electronegativity

A

The power of an atom to attract a pair of electrons towards itself
In a covalent bond

42
Q

Explain in terms of electronegativity why the boiling point of H2S2 is lower than H2O2

A

Electronegativity of S is lower than O / Smaller electronegative difference between H and S is lower
No hydrogen bonding in H2S2 molecules as they only have van de waals forces

43
Q

Suggest why electronegativity increases from lithium to fluorine

A

Number of protons increase so they have a stronger nuclear charge
They have same shielding
So atoms get smaller

44
Q

Describe why bonding in nitrogen oxide is covalent rather than ionic

A

Small electronegativity difference

45
Q

Explain how strongest type of intermolecular force arises between two molcules of ammonia

A

Large electronegativity difference between N and H
Dipoles are created as Form N (delta negative) and H (delta positive)
Lone pair on nitrogen forms a weak bond with Hydrogen

46
Q

Suggest why boiling point of AsH3 is lower than that of NH3

A

NH3 has hydrogen bonding and AsH3 has weak van de waals forces
More energy needed to break hydrogen bonds

47
Q

Describe bonding in a crystal of iodine

A

Covalent bonds between atoms
VDW forces between molecules

48
Q

Describe why heat energy is required to melt an iodine crystal

A

Bonds between molecules must be broken

49
Q

State type of bonding between molecules of HCl and explain how this arises

A

Permanent dipole - dipole
This arises as there is a difference in electronegativity which leads to bond polarity
Dipoles dont cancel out and therefore molecule has an overall permanent dipole
there is an attraction between delta positive of one molecule and delta negative of another molecule

50
Q

State why Hydrogen iodide requires more heat energy for melting than does hydrogen chloride

A

HI is a bigger molecule / has more electrons
So it has stronger forces between its molecules

51
Q

State why hydrogen bromide has a higher melting point than hydrogen chloride

A

Hydrogen bromide molecule is bigger so it has stronger van de waals forces
Van de waals dforces increase with size / Mr

52
Q

State type of intermolecular force in SiF4. Explain how this type of intermolecular force arises

A

Van de waals forces
Electron movement in molecule causes uneven distribution of electrons
This induces a dipole in another molecule
Symmetrical molecule so dipoles cancel
Delta positive attracts delta negative in different / adjacent molecules

53
Q

Explain in terms of bonding why fluorine has a low boiling point

A

vdw forces between molecules
are weak and need little energy to overcome

54
Q

Boiling point of iodomethane is higher than that of fluoromethane. Explain why

A

Iodine is bigger than fluorine so vdw forces between iodomethane molecules are stronger than the vdw forces between the fluoromethane molecules.
Dipole - dipole forces between fluoromethane are stronger than those of iodomethane
Vdw forces between iodomethane is stronger than the dipole dipole forces fluromethane

55
Q

In terms of intermolecular forces suggest why phosphine (PH3) is almost insoluble in water

A

Does not form hydrogen bonds with water

56
Q

State whether aluminium can conduct electricity when solid or molten

A

Both because it has delocalised electrons

57
Q

State whether alumium fluoride conducts electricity when solid or molten

A

Aluminium fluoride conducts when molten because it has mobile electrons.
Aluminium fluoride doesnt conduct when solid as alumium fluoride ions which are fixed so ions are not mobile as it is an ionic lattice

58
Q

State whether boron tribromide can conduct electricity when solid or molten

A

Boron tribromide does not conduct in solid and molten states as it has no delocalised electrons

59
Q

Suggest why titanium can be hammered into different shapes with similiar strengths

A

Strong metallic bonding remains the same
The same attraction, same bond strength and same crystal structure remains between protons and delocalised electrons

60
Q

Phosphine (PH3) molecules contain hydrogen atoms, suggest why there is no hydrogen bonding between phosphine molecules

A

Difference in electronegativity between P and H is too small

61
Q

Write an equation for formation of aluminium chloride from its elements

A

Al +1.5Cl2 -> AlCl3

62
Q

Aluminium chloride has a molecular mass of 267 in as phase
Deduce formula of aluminium compound that has relative molecular mass of 267

A

Al2Cl6

63
Q

Deduce formula of a compound that has same number of atoms, same number of electrons, and same shape as AlCl4^-

A

SiCl4

64
Q

Deduce empirical formula of graphane

A

CH

65
Q

State element in period 3 that has the highest melting point

A

Silicon
it has macromolecular structure
it has many strong covalent bonds which require a lot of energy to break

66
Q

Mp of magnesium is 923 and bp of Mg is 1383
Mp of bromine 266 and bp of bromine is 332
Suggest why magnesium is a liquid over a much greater temperature range

A

Mg has much greater liquid range because forces of attraction in liquid / molten metal are stronger compared to forces in Br2

67
Q

Write an equation for the reaction of phosphorus with an excess of oxygen

A

P4 + 502 -> P4O10

68
Q

Write an equation for reaction of sulfur trioxide and with potassium hydroxide

A

SO3 +2KOH -K2S04 + H20

69
Q

Explain why SbCl3 molecules are polar

A

There is a difference in electronegativity so the bonds are polar and have p.d.d
Molecule is not symmetrical as dipoles do not cancel

70
Q

In terms of structure and bonding explain why calcium has a higher melting point than potassium

A

Both have giant metallic lattice structure with strong electrostatic attractions between positive ions and delocalised electrons
Calcium has a greater ionic charge than potassium and has more delocalised electrons
Therefore stronger metallic bonds and more energy required to break them

71
Q

What is the formula of calcium nitrate (v)

A

Ca(NO3)2

72
Q

Which compound has the highest boiling point
1. CH3CH2CH2OH
2. CH3CH2CHO
3. CH3COCH3
4. CH3COOCH3

A
  1. CH3CH2CH2OH

only 1 and 2 have hydrogen bonding and 1 has more electrons / larger mr / larger size

73
Q

Explain trend in electronegativity down the halogen group

A

Decreases
Atomic radius increases
So decreasing attraction of protons for shared pair of electrons

chemistry (10 decks)

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