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Chemistry > Structure + Bonding > Flashcards

Structure + Bonding Flashcards

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0
Q

Elements with the … Number of electrons on the … Shell have … … Properties

A

Same
Outer
Similar
Chemical

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1
Q

How are ions similar and different in the periodic table

A

Similar: react the same because same electrons in outer shell
Different: react different because more shells down the group in group 1

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2
Q

The relationship between group number and electronic configuration is shown in the table

A 
Group | no electrons out shell | ion charge
1  1  +1
2  2  +2
3  3  +3
4  4  X
5  5  -3
6  6  -2
7  7  -1
8  2/8  X
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3
Q

The element in group 4 and 8(0) generally do not…

A

Form ions

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4
Q

Noble gases are unreactive because their atoms …

A

Have stable electronic arrangements

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5
Q

Atoms other than noble gases can achieve stable electronic structures by … Or … Electrons to form ions ( or … Electrons to form … Bonds)

A

Gaining
Losing
Sharing
Covalent

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6
Q

Positive and negative ions … To form … Bonds

A

Attract

Ionic

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7
Q

Ionic bonds hold … Charged ions together in … Structures. Strong electrostatic forces of attraction act in … Directions.

A

Oppositely
Giant
All

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8
Q

Each ion in the lattice is … By ions with the … Charge and so is held … In place

A

Surrounded
Opposite
Firmly

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9
Q

Draw a sodium chloride crystal

A

On paper

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10
Q

A lot of … is needed to … the ionic bonds to melt the solids so ionic compounds have … melting and boiling point

A

Energy
Overcome
High

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11
Q

… ionic compounds … conduct electricity as the ions are held firmly in place by strong electrostatic forces

A

Solid

Cannot

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12
Q

When ionic compounds are … in water the ions are … from one another by the water molecules. They are then … to move in solution, are able to … charge and therefore able to … electricity.

A 
Dissolved
Separated 
Free
Carry
Conduct
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13
Q

When ionic compounds are melted they are … To conduct electricity as the ions are … To move and are able to … Electrical charge

A

Able
Free (sea of delocalised electrons)
Carry

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14
Q

What is the representation of a sodium chloride called

A

Giant lattice structure

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15
Q

Giant Covalent bonding

A
  • Non metal to non metal
  • these structures contain many strong covalent bonds (diamond)
  • high melting points
  • doesn’t conduct electricity
  • not soluble in water
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16
Q

Ionic bonding

A
  • Non metal to metal
  • gaining or losing electrons to achieve a full outer shell
  • high melting points
  • cannot conduct electricity
  • soluble in water
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17
Q

Metallic bonding

A
  • Metal to metal
  • lattice structure of metal ions with outer shell electrons free to move through the structure
  • high melting point
  • conducts electricity
  • not soluble in water
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18
Q

Covalent bonding is the … Of attraction between a… And the … Of the adjacent atoms

A

Electrostatic force
Shared pair of electrons
Nucleus

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19
Q

Strong covalent bonds exist between atoms to form … molecules. The force of attraction between these molecules is very weak (AKA …) things that have low melting points have a … covalent bond.

A

Small
Intermolecular forces of attraction
Simple

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20
Q

Name 3 properties, uses and the structures of graphite

A
  • Layers slide over each other, lubricant and pencil lead, forms flat sheets of covalently bonded structures which are stacked on top of each other but held together by weak non covalent interactions
  • conducts electricity, electrodes, as there is a vast delocalisation within the carbon layers which have free electrons so are able to conduct electricity
  • very high melting point, crucible for holding molten metal, the bonds holding together the layers (intermolecular bonds) are very strong and requires a lot of energy to separate
21
Q

Name 3 properties, uses and structures of a diamond

A
  • doesn’t conduct electricity, insulating material, no free electrons to carry electricity current as all of its valence electrons are involved in bonding
  • hardest material known, cutting tools and drills, has most stable atomic structure which makes it more difficult to remove molecules
  • very high melting point, jewellery, strong carbon covalent bonds which is considered as a stone with superlative physical qualities as contains bonds which are extremely hard to break
22
Q

Diamonds and graphite both only contain … And are … Of each other

A

Carbon

Allotropes

23
Q

Metallic bonding properties

A
  • high melting and boiling points: as they have powerful attractions so a lot of energy is required to separate them
  • conduct electricity: this is because the delocalised electrons are free to move throughout the structure
  • malleable: easily beaten into shape
  • ductile: easily pulled into wires
24
Q

Simple molecular (covalent) bonding

A
  • non metal to non metal
  • electrostatic force of attraction between a shared pair of electrons
  • low melting points
  • cannot conduct electricity
  • insoluble
25
Q

Cation and anion difference

A

Cation is positive

Anion is negative

26
Q

Hydroxide charge and symbol

A

-1

OH

27
Q

Nitrate charge and symbol

A

-1

NO3

28
Q

Carbonate charge and symbol

A

-2

CO3

29
Q

Sulphate charge and symbol

A

-2

SO4

30
Q

Sulphite charge and symbol

A

-2

SO3

31
Q

Solid structure

A

Tight, uniform, small vibrations, strong forces of attraction between them

32
Q

Liquid structure

A

Moulds to its container, particles still touching a bit with some gaps, less dense than solids, forces of attraction are weaker

33
Q

Gas structure

A

Very far apart, not uniform structure, basically no forces of attraction between them

34
Q

When a solid turns to liquid

A

Melts at its melting point, vibrations become stronger an stronger until forces of attraction are no longer strong enough to hold them together

35
Q

When a liquid turns to a gas (evaporation)

A

Some fast particles on the surface of the liquid will have enough energy to break away from the gas

36
Q

When a gas turns to a liquid

A

Condensation, when gas is cooled the particles eventually move slowly enough that attractions between them hold as a liquid

37
Q

When a liquid turns to a solid

A

Solidification, particles start to move slowly until so slow that forces of attraction can hold them together in a solid

38
Q

Solid to gas and vice versa

A

Sublimation, no ability to be in a liquid state

39
Q

When a liquid turns to a gas (boiling)

A

When the liquid is heated so strongly that the particles are moving fast enough to break all forces of attraction, bubbles of gaseous particles are formed throughout the liquid and rise to the surface

40
Q

A gas can diffuse between others, describe it vertically and horizontally

A

Vertically - quickly if denser gas on top

Horizontally - slowly and diffuse not in the middle but on the side of denser gas

41
Q

Dilution of strongly coloured solution like potassium manganate and water

A

Takes days for the colour to diffuse throughout the whole water as only smalls gaps between the liquid particles for other particles to diffuse into

42
Q

Diffusion of bromine particles and air

A

Can diffuse very easily, the brown colour will diffuse upwards or sideways until all the colours are light brown, boh particles bounce around constantly to give an even mixture

43
Q

Define an atom

A

the smallest component of an element having the chemical properties of the element, consisting of a nucleus containing combinations of neutrons and protons and one or more electrons bound to the nucleus by electrical attraction; the number of protons determines the identity of the element.

44
Q

Define a molecule

A

the smallest physical unit of an element or compound, consisting of one or more like atoms in an element and two or more different atoms in a compound.

45
Q

Define an element

A

one of a class of substances that cannot be separated into simpler substances by chemical means

46
Q

Define a compound

A

a pure substance composed of two or more elements whose composition is constant.

47
Q

Define a mixture

A

two or more substances that are not chemically united and that exist in no fixed proportion to each other

48
Q

Atom structure

A

Nucleus made up of protons and neutrons

Electrons found in large distance from the nucleus orbiting it

49
Q

Relative charge and mass for a neutron

A

Charge - 0

Mass - 1

50
Q

Relative charge and mass for an electron

A

Charge - -1

Mass - 0

51
Q

Relative charge and mass for a proton

A

Charge - +1

Mass - 1

Chemistry (11 decks)

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