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Higher Chemistry > Periodicity > Flashcards

Periodicity Flashcards

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1
Q

What bonds are covalent

A

strong bonds

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2
Q

what is monoatomic

A

noble gases that don’t bond

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3
Q

how is the elements in the periodic arranged?

A

increasing proton number but took into account similar properties

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4
Q

What does high values of periodicity indicate?

A

a lot of energy is needed to separate the particles

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5
Q

what are intermolecular bonds?

A

bonds between two atoms

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6
Q

what are intramolecular bonds?

A

bonds inside an atom

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7
Q

what type of bonds are between noble gases?

A

weak bonds

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8
Q

why do carbon and silicon have a high melting value?

A

they are covalent networks and have a strong attraction as they want to gain 4 electrons

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9
Q

why is the size of an atom very difficult to measure?

A

it doesn’t have a distinct edge

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10
Q

how is the bond length measured?

A

the nuclei of an atom to the nuclei of the other atom

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11
Q

what is the covalent radius?

A

half the distance between the nuclei of two of its

covalently bonded atoms.

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12
Q

what happens to the atomic size going along a period?

A

as it goes along a period the atomic size decrease as the nuclear charge is stronger so it pushes the electrons closer together

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13
Q

what happens to the atomic size going down a group?

A

the atomic size increases as it has an extra outer energy level of the occupied shells and the electrons to the nucleus is further apart.

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14
Q

what is the screening effect?

A

there is more outer shell between the nucleus and electrons so there is less attraction

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15
Q

why do noble gas don’t have a covalent radius?

A

They don’t have bonds as they are stable

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16
Q

What is ionisation energy?

A

the energy required to remove one mole of electrons from one mole of gaseous atoms

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17
Q

As you go along a period what happens to the ionisation number?

A

the nuclear charge between the protons and electrons are stronger and more attraction so the ionisation number increases

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18
Q

As you go down a group what happens to the ionisation energies?

A

The ionisation energy decreases as the electrons ,are further apart from the nucleus therefore the attraction isn’t as strong (screening effect)

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19
Q

What is electronegativity?

A

Measure of an atom’s attraction for the shared pair of electrons in a bond

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20
Q

What happens to the electronegativity as you go across a period?

A

It increases as it has more protons which is because it has an increase in nuclear charge

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21
Q

What happens to the electronegativity as you go down a group?

A

the electrons are further apart from the protons so the attraction isn’t as strong as there is more outer shells.
The screening effect prevents the electrons to nucleus so attraction isn’t as attraction

22
Q

What is a covalent bond?

A

the attraction between the positive nucleus and the delocalised electrons

23
Q

why can graphite conduct electricity?

A

because it has a delocalised electron as it only forms 3 bonds so has one bond left

24
Q

what elements in the first 20 have a covalent network substance?

A

Boron, carbon and silicon

25
Q

why can diamond not carry out electricity?

A

because it forms 4 bonds with carbon atoms so it has no delocalised electrons

26
Q

why is diamond the hardest natural substance?

A

because it has 4 strong bonds

27
Q

why is graphite soft and flaky?

A

It has weak bonds and is in layers

28
Q

what is a use of diamond?

A

the tip of drill contains diamond to cut through glass or tiles

29
Q

Why is graphite used as an industrial lubricant?

A

It has layers so it is easy to move the weak bond s

30
Q

what bond is a fullerene (c60) atom?

A

covalent molecular

31
Q

what is a covalent bond?

A

bonds forms when a pair of electrons are shared between the two atoms

32
Q

what is pure covalent ?

A

when atoms in a covalent bond have the same electronegativity

33
Q

what is polar covalent?

A

when atoms in a covalent bond have different electronegativity

34
Q

why does tin(IV) iodine and titanium tetrachloride have a low melting point?

A

they have a low melting point which indicates the bonding is covalent

35
Q

What are the london dispersion forces of the van der waals forces?

A

the weakest forces

36
Q

What is a temporary dipole?

A

when there is a positive and negative side in a monatomic bond which lasts for a short time

37
Q

What is an induced dipole?

A

Its when a temporary dipole cause another atom to form a temporary dipole

38
Q

What happens to the london dispersion forces going down a group?\f

A

The melting and boiling point increases due to the increase of electrons and the attraction is stronger

39
Q

How are permanent dipole permanent dipole interactions different to london dispersion forces?

A

permanent dipole interactions are stronger

40
Q

Are london dispersion forces still present with a permanent dipole-permanent dipole interactions?

A

yes

41
Q

Why do permanent dipole-permanent dipole interactions have a higher boiling point than molecules with london dispersion forces?

A

It has stronger forces and greater attraction so it requires more energy to break the bonds

42
Q

what is an experiment to see if its polar?

A

A charged rod placed next to the liquid and if it was polar it would bend

43
Q

what are the molecules that can form hydrogen bonds?

A

Nitrogen,Oxygen and fluorine

44
Q

what happens to the volume and density when liquid water cools?

A

the volume of water increases and it expands and the density decreases

45
Q

what happens to the hydrogen bonds in ice?

A

the bonds become stronger so they don’t break and the molecules become further apart

46
Q

why does ice float on water?

A

Ice is less dense than water

47
Q

what is viscosity a measure of?

A

how thick a liquid is

48
Q

How is london dispersion forces formed?

A

when an atom that has electrons that are at one side of the molecule so it has a partial negative and positive side which causes a temporary dipole

49
Q

How is temporary dipole temporary dipole interactions formed

A

It only happens with polar molecules because of their difference in their electronegativity so it has a positive and negative side which is permanent.

50
Q

How is hydrogen bonding formed

A

it is when hydrogen is attached to either Nitrogen, oxygen or fluorine is really strong because of their difference in electronegativity.

Higher Chemistry (8 decks)

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