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Chemistry 🧪 > Atomic structure and bonding (2) ✅ > Flashcards

Atomic structure and bonding (2) ✅ Flashcards

1
Q

What did John Dalton do?

A

-all elements are made up of small indivisible particles called atoms
-atoms cannot be created or destroyed
-atoms of different elements have different properties

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2
Q

what did j.j thompson do?

A

-discovered the electron
-proposed the plum pudding model
-suggested atom was neutral as it contained equal number of protons and electrons

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3
Q

what is the plum pudding model

A

negative electrons embedded into a sphere of positive charge

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4
Q

what did ernest rutherford do?

A

-proved that atoms consisted of electrons revolving around positively charged nucleus
-called the positive particles protons

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5
Q

what did james chadwick do?

A

-showed the nucleus of the atom contained two different types of particles
-neutral particles are called neutrons
-they were difficult to detect because it had no charge

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6
Q

what is the relative mass of a proton

A

1

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7
Q

what is the relative mass of a neutron

A

1

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8
Q

what is the relative mass of an electron

A

1/1840

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9
Q

what is the relative charge of a proton

A

+1

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10
Q

what is the relative charge of a neutron

A

0

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11
Q

what is the relative charge of an electron

A

-1

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12
Q

where is the proton found

A

in the nucleus

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13
Q

where is the neutron found

A

in the nucleus

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14
Q

where is the electron found

A

in the shell

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15
Q

what is the atomic number

A

number of protons in an atom

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16
Q

what is the mass number

A

protons + neutrons

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17
Q

why does the atom as a whole have no electrical charge

A

the number of protons and neutrons are equal so the charges cancel out

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18
Q

what does the group number represent
(the number of _________ in the outer _____)

A

the number of electrons in the outer shell

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19
Q

what does the period number represent
(number of ______ in use)

A

number of shells in use

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20
Q

what is the size of an atom

A

0.1 nanometers

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21
Q

what’s an isotope

A

isotopes are atoms of an element with the same atomic number but a different mass number, therefore a different number of neutrons

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22
Q

what do all noble gasses have

A

stable full outer shell of electrons

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23
Q

what are ions and how are they formed

A

charged particles formed when atoms lose or gain electrons to achieve a full outer shell of electrons

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24
Q

if an atom gains an electron does it become positive or negative

A

negative

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25
Q

what are molecular ions

A

charged particles containing more than one atom

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26
Q

in this carbonate ion, where is the valency
2-
CO
3

A

-2

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27
Q

what is chemical bonding

A

when an atom doesn’t have a full outer shell, it will want to react with another atom to achieve a full outer shell

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28
Q

what are the three types of bonding

A

Ionic bonding
Covalent
Metallic

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29
Q

ionic bonding is between what two types of elements

A

metal + non-metal

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30
Q

covalent bonding is between what two types of elements

A

non-metal + non-metal

31
Q

metallic bonding is between what two types of elements

A

metal + metal

32
Q

when do ionic bonds form

A

when a metal transfers electrons to a non-metal forming positive and negative ions

33
Q

where is ionic bonding found

A

in metal compounds

34
Q

what is a crystal of sodium chloride held together by?

A

a giant ionic lattice

35
Q

physical properties of ionic compounds

A

high melting/boiling point
soluble in water
DONT HAVE electrical conductivity UNLESS MOLTEN OR DISSOLVED IN WATER

36
Q

why do substances of ionic compounds have a high melting/boiling point

A

lots of energy is required to break the STRONG ELECTROSTATIC FORCES OF ATTRACTION as a result ionic substances are solid at room temp and have high b/m point

37
Q

why do substances of ionic compounds have no electrical conductivity

A

because there are no charged particles free to move and carry the charge

38
Q

what is covalent bonding

A

a covalent bond is a shared pair of electrons the bonds within the molecules are strong and require lots of energy to break them

39
Q

where is covalent bonds found in

A

found in non-metallic elements and compounds

40
Q

what are covalent substances composed of and what are they called and what is their structure described as

A

small molecules called simple covalent molecules. structure described as molecular covalent

41
Q

what are the weak intermolecular forces of attraction between the covalent structures molecules called

A

Van der Waals’ forces

42
Q

what are the physical properties of molecular covalent structures

A

low melting/boiling points
don’t conduct electricity
insoluble in water

43
Q

why do molecular covalent structures have low melting/boiling points

A

little energy is required to break the weak Van der Waals’ forces of attraction between the molecules

44
Q

what do molecular covalent structure substances exist as at room temperature

A

gasses, liquids or low melting point solids

45
Q

why do molecular covalent structure substances not conduct electricity

A

they have no charged ions or electrons to move and carry the charge

46
Q

what are giant covalent structures composed of

A

covalently bonded atoms

47
Q

properties of giant covalent structures (2)

A

high melting/boiling point
insoluble in water

48
Q

why do giant covalent structures have high melting/boiling points

A

the many strong covalent bonds between the atoms means a lot of energy is required to break the strong covalent bonds

49
Q

name a use of diamonds

A

diamond tipped drills to cut through things like rock, metal and glass

50
Q

Property of diamond (carbon)

Each carbon atom is covalently bonded to 4 other carbon atoms in what arrangement for diamond?

A

in a tetrahedral three-dimensional arrangement

51
Q

Name two properties of diamond other than the arrangement/what its bonded to

A

doesn’t conduct electricity
high melting point

52
Q

name two uses of graphite and why graphite is used for them

A

lubricant for machinery
pencil leads

because layers can slip easily over one another

53
Q

property of graphite (carbon)

what arrangement are graphite atoms arranged in, and to how many other carbons is it bonded to? The layers are held together by what + what are they caused by, which can easily …. …. ………
therefore…

A

in the hexagonal layers each carbon is bonded to 3 others. The layers are held together by weak forces caused by delocalised electrons which can easily slip over each other. Therefore graphite is a soft substance

54
Q

name two other properties of graphite (carbon)

A

conducts electricity
high melting point

55
Q

why does graphic (carbon) conduct electricity

A

the delocalised electrons between layers are free to move and carry charge

56
Q

what are allotropes, their state

A

different forms of the same element in the same physical state

57
Q

name 3 examples of allotropes

A

Diamond, graphite, graphene - forms of the same element
carbon - same physical state (solid)

58
Q

what is the arrangement of metallic bonding

A

regular arrangement of positive ions surrounded by a sea of delocalised electrons

59
Q

what is the metallic bond

A

the strong force of attraction between the positive metal ions in a regular lattice and the delocalised electrons

60
Q

Name 3 properties of metals

A

High melting point
Conduct electricity
Malleable
Ductile

61
Q

why do metals have a high melting point

A

a large amount of energy is required to break the strong metallic bonds between the positive ions and the delocalised electrons

62
Q

all metals are solids, the only exception is m……

A

mercury

63
Q

if a metal is solid at room temperature that means it has a high ….
(2)

A

boiling and melting point

64
Q

why are metals malleable and ductile?

the layers can slide over
without disrupting the
the ……. is maintained because
after sliding the positive ions settle into their new ……… and what is restored

A

the layers of ions can slide over each other without disrupting the bonding, the bonding is maintained because the bonds are fixed and not rigid. after sliding the positive ions settle into their new positions and structure is restored

65
Q

what is an alloy and what is the resulting mixture

A

mixture of two or more elements one of which is a metal. Resulting mixture has metallic properties

66
Q

what are the improved properties of an alloy and an example
(mild steel is an alloy of)

A

hardness
electrical conductivity
resistance to corrosion

mild steel is an alloy of iron and carbon

67
Q

how do you work out the percentage of gold in an alloy?

A

number of carats
————————- X100
24

68
Q

what is a use of aluminium + why aluminium is used for that

A

overhead electrical wires

conducts electricity, low density, malleable + ductile

69
Q

what are 2 uses of magnesium + why magnesium is used for them

A

flares and airplanes

burns with bright white light, strong, low density

70
Q

what is a use of iron + why iron is used for them

A

bridges and structures

strong, relatively cheap

71
Q

what is a use of copper + why is copper used for it

A

plumbing applications

doesn’t react with water/steam, malleable, ductile

72
Q

what is a nanoparticle

A

a structure 1-100nm in size and contains a few hundred atoms

73
Q

how do you work out RAM/AR

A

(mass of isotope x abundance)
+
(mass of isotopes x abundance
————————————————
Total abundance

74
Q

why is the mass number of chlorine given as 35.5 in the periodic table if the mass of one isotope is 35 and the other is 37?

A

Isotopes don’t occur in equal amounts
-75% of chlorine atoms have a mass of 35
-25% of chlorine atoms have a mass of 37

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