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chemistry > chemical bonding, structure and physical properties of substances > Flashcards

chemical bonding, structure and physical properties of substances Flashcards

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1
Q

where is ionic bonding formed

A

between metal and non-metal atoms

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2
Q

ionic bonding definition

A

strong electrostatic attraction between positive and negative ions

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3
Q

structure of ionic bonding

A

giant ionic structure

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4
Q

what does the ionic bonding structure consist of?

A

continuously repeating 3-dimensional lattice of positive and negative ions

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5
Q

melting and boiling point of ionic compounds

A

high melting, boiling point.
explanation: large amount of heat energy is needed to break the strong ionic bonds.

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6
Q

electrical conductivity of ionic compounds

A

conductor of electricity in molten and aqueous state.
explanation: in solid state, the ions are not free-moving. in molten or aqueous state, the ions are free moving and hence can conduct electricity.

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7
Q

solubility (in water/organic solvent) in ionic compounds

A

soluble in water, insoluble in organic solvents

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8
Q

where is covalent bonding formed?

A

between non-metal atoms

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9
Q

definition of covalent bonds

A

strong bond that is formed by the sharing of electrons

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10
Q

one pair of shared electrons is represented by ‘—‘. what is this known as

A

single covalent bond

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11
Q

what is simple covalent? give examples

A

covalent bonds among few atoms, H2, H2O, NH3, CH4, CO2

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12
Q

what is giant covalent? give examples

A

covalent bonds among large number of atoms. diamond, silicon, graphite.

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13
Q

what does the simple covalent structure consist of?

A

many molecules

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14
Q

what are the molecules in simple covalent substances attracted together by?

A

weak intermolecular forces

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15
Q

within each molecule, what are between atoms in simple covalent bonding?

A

strong covalent bonds

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16
Q

what is the structure of simple covalent substances known as?

A

simple covalent structure

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17
Q

melting and boiling point of simple covalent substances

A

low melting and boiling point
explanation: small amount of heat energy is needed to break the weak intermolecular forces
note** when melting or boiling simple covalent substances we are breaking the weak intermolecular forces and not the covalent bond between the atoms.

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18
Q

electrical conductivity of simple covalent substances, explain

A

non-conductor of electricity in any states
explanation: there are no free-moving electrons to conduct electricity

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19
Q

solubility of simple covalent substances

A

insoluble in water, soluble in organic solvents

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20
Q

what does the structure of giant covalent substances consist of

A

it consists of atoms forming covalent bonds throughout the entire structure

21
Q

what is the structure of giant covalent substances known as?

A

giant covalent structure

22
Q

examples of giant covalent substances

A

diamond, graphite, silicon, silicon dioxide

23
Q

in the structure of diamond, each carbon atom form covalent bond with how many other carbon atoms throughout?

A

4

24
Q

what arrangement/shape does the bonding between atoms in diamond result in

A

tetrahedral arrangement/shape

25
Q

melting and boiling point of diamond

A

high melting and boiling point
explanation: large amount of heat energy is needed to break the strong covalent bonds

26
Q

electrical conductivity of diamond

A

does not conduct electricity
explanation: there are no free-moving (mobile) electrons to conduct electricity. (each carbon atom in diamond used all outer electron in bonding.

27
Q

solubility of diamond

A

insoluble in both water and organic solvents

28
Q

hardness of diamond

A

very hard because of the strong covalent bonds keeps the carbon atoms in fixed position when force is applied.

29
Q

uses of diamond

A

tips of drilling or cutting tools

30
Q

in the structure of graphite, each carbon atom forms covalent bonds with how many other carbon atoms

A

3

31
Q

what arrangement/shape does the bonding between atoms results in graphite

A

hexagonal arrangement/shape

32
Q

the many layers of graphite are held together by what

A

weak intermolecular forces

33
Q

melting and boiling point of graphite

A

high melting and boiling points
explanation: large amount of energy is needed to break the strong covalent bonds

34
Q

electrical conductivity of graphite

A

can conduct electricity
explanation: there are free-moving (mobile) electrons to conduct electricity

35
Q

solubility of graphite

A

insoluble in water and organic solvents

36
Q

hardness of graphite

A

soft and slippery
explanation: the layers of carbon atoms are able to slide over one another when a force is applied.

37
Q

uses of graphite

A

in pencil lead
as a solid lubricant to reduce friction in machinery
in brushes for electric motors and as electrodes

38
Q

state the type of structure silicon belongs to

A

giant covalent structure

39
Q

state the properties of silicon
- melting and boiling point
- electrical conductivity
- hard or soft solid
- solubility in water and organic solvents

A
  • high melting and boiling point
  • poor conductor of electricity
  • hard solid
  • insoluble in water and organic solvents
40
Q

state the type of structure silicon belongs to

A

giant covalent structure

41
Q

state the properties of silicon
- melting and boiling point
- electrical conductivity
- hard or soft solid
- solubility in water and organic solvents

A
  • high melting and boiling points
  • non-conductor of electricity
  • hard solid
  • insoluble in water and organic solvents
42
Q

metal atoms in the structure loses their valence electron and form what?

A

positive ions

43
Q

the valence electrons are __________ , giving rise to ____________.

A

free-moving, ‘sea’ if delocalised valence electrons

44
Q

what does the attraction between the positive metal ions and the mobile electrons result in?

A

metallic bonding

45
Q

definition of metallic bonding

A

strong electrostatic attraction between the metal ions and the delocalised valence electrons

46
Q

melting and boiling point of metals

A

high melting and boiling point
exception: mercury is a liquid at room temperature
explanation: large amount of heat energy is needed to break the strong metallic bonds

47
Q

electrical conductivity of metals

A

metals can conduct electricity in all states
explanation: there are free-moving (mobile) electrons present to conduct electricity.

48
Q

solubility of metals

A

insoluble in water and organic solvents
note** some metals react with water to form compounds

49
Q

lattice definition

A

it refers to a regular three-dimensional, orderly arrangement of particles

chemistry (1 decks)

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