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CHEM👑 > Topic 3 > Flashcards

Topic 3 Flashcards

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1
Q

Does atomic radius increase or decrease down a group?

A

increase

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2
Q

Why does atomic radius increase down a group

A
  • the addition of protons causes an increase in nuclear charge & this causes the electrons to experience stronger electrostatic forces of attraction
  • each member of the group has 1 more electron shell than the previous element, this increases the electron-electron repulsion
  • each electron shell is located further away from the nucleus
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3
Q

Does atomic radius increase or decrease across a period?

A

decrease

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4
Q

Why does atomic radius decrease across a period?

A
  • the number of protons (7 hence nuclear charge), & number of electrons increase by 1 w each successive element
  • the additional electron added to the atom occupies the same main energy level
  • this means that the electron-electron repulsion only increases slightly
  • the greater electrostatic attraction force exerted by the increasing pos nuclear charge pulls the electrons in closer to the nucleus
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5
Q

What is a cation?

A

atom w contains fewer electrons than protons

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6
Q

are cations smaller or larger than the original atom? And y?

A
  • smaller
    has fewer electrons than protons, so the electrostatic attraction between the nucleus & all the electrons is greater making it smaller
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7
Q

What do melting points of an element depend on?

A
  • structure of the element

- type of attractive forces holding the atoms/molecules together

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8
Q

Does ionisation energy increase or decrease within a group?

A

decreases within a group bc the electron being removed is in a shell which is located progressively further from the nucleus.

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9
Q

why does Ionisation energy decrease down a group

A
  • the nuclear charge increases w increasing atomic number, so there are greater attractive forces between the nucleus and outer electrons - more energy is required to overcome attractive forces when removing an electron
  • electrons in shells that are further away from the nucleus are less attracted to the nucleus so the further the outer electron shell is from the nucleus, the lower the ionisation energy
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10
Q

does ionisation across a period increase or decrease?

A

increase

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11
Q

Why does ionisation energy increase across a period?

A
  • the nuclear charge increases
  • distance between the nucleus and outer electron remains reasonably constant
  • there is a decrease between groups 2 and 3 because elements of group 3 contain one extra electron in a p orbital, compared with those in group 2.
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12
Q

Does electronegativity increase or decrease down a group?

A

decreases

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13
Q

Does electronegativity increase or decrease down a period?

A

increases

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14
Q

Why does electronegatively decrease down a group?

A
  • attraction between the outer (valence) electrons and the nucleus increases as the atomic radius decreases in a period
  • electronegativity values decrease with an increase in atomic radii down a group
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15
Q

what are the properties that increase w increasing electronegativity?

A

non-metallic properties

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16
Q

Why does electronegatively increase down a period?

A

electronegativity decreases as you go down a group as electrons are further away from the nucleus, smaller attractive force

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17
Q

Does electron affinity increase or decrease down a group?

A

decrease

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18
Q

what type of reactions can all halogens do?

A

The halogens are all oxidising agents and displacement (replacement) reactions can take place between them. Would the following reaction occur?

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19
Q

do elements in the same group have similar properties?

A

yes

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20
Q

State the trend in reactivity down group 17 (from top to bottom)

A

decreases

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21
Q

What best describes the oxide of aluminium?

A

Amphoteric

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22
Q

are metal oxides basic or acidic?

A

basic

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23
Q

are non-metal oxides basic or acidic?

A

acidic

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24
Q

what is the name given to group 18 elements

A

noble gases

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25
Q

What happens when a basic oxide reacts w an acid?

A

A basic oxide will react with an acid to form salt and water only.

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26
Q

Oxides of reactive metals may react with what? to form what?

A

water to form a basic solution

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27
Q

An acidic oxide will react with a base to form what?

A

An acidic oxide will react with a base to form a salt and water only.

28
Q

Some oxides of non-metals will react with what? to form what?

A

Some oxides of non-metals will react with water to form an acidic solution.

29
Q

is aluminium oxide soluble or insoluble in water?

A

insoluble

30
Q

are group 1 compounds soluble or insoluble in water?

A

soluble

31
Q

Reactions of group 1 elements

A
  • All the group 1 elements react rapidly with water releasing hydrogen and forming alkaline solutions
  • The oxides are basic and react with water to form solutions of the hydroxides
  • strong reducing agents and react with most non-metals
    forming ionic compounds
32
Q

What are reducing agents

A

Reducing agents are substances that release electrons and cause another substance to be reduced

33
Q

which group consists of the diatomic molecules?

A

halogens, group 17

34
Q

Which element is the weakest oxidising agent in group 17?

A

iodine is the weakest oxidizing agent so it has the least tendency to form negative ions.

35
Q

In group 17 what does a more reactive halogen do?

A

In group 17 a more reactive halogen displaces a less reactive halogen in a redox reaction. The order of reactivity (oxidizing strength) for the halogens is Cl > Br > I

36
Q

what do displacement reactions involve?

A

an electron transfer

37
Q

inert definition

A

unreactive

38
Q

Properties of noble gases

A
  • melting & boiling points are very low bc the London forces are extremely small.
  • They increase as the group is descended bc there are more electrons that are easily polarised on the outside of the atoms
  • elements are monoatomic
  • their ionisation energies are too high for them to form cations. However, xenon can use its d orbitals to form bonds with fluorine and oxygen.
39
Q

Why are non-metal ions acidic?

A

bc they form hydrogen ions in aqueous solutions

CO2 + H20 —> H2CO3 (carbonic acid)

40
Q

What are non-metal oxides?

A

Non metal oxides are covalent bonds between non metals and oxygen
- carbon monoxide

41
Q

What are metal oxides?

A

Metal oxides are crystalline solids that contain a metal cation and an oxide anion
- sodium oxide

42
Q

Why are metal oxides basic?

A

Metal oxides are basic because they form hydroxides in aqueous solutions
Na2O + H2O —> 2NaOH

43
Q

What does metallic character refer to?

A

the reactivity of a metal
- It depends on the ability of an element to loose its valence electrons

  • metallic character increases down a group
    • increased ability to lose electrons makes them more reactive
  • metallic character decreases across a period
44
Q

What does non-metallic character refer to?

A

the reactivity of a non metal
- It depends on the ability of an element to accept electrons

  • non metallic character decreases down a group
    • decrease in electron affinity due to increase in atomic size
  • non metallic character increases across a group
    • increase in electron affinity due to decrease in atomic size
45
Q

What are amphoteric oxides?

A

Metal oxides which react with both acids as well as bases to produce salts and water are known as amphoteric oxides, the reactivity of a substance with both acids and bases, acting as an acid in the presence of a base and as a base in the presence of an acid.

46
Q

Definition of periodicity

A

repeating pattern of physical & chemical properties seen at regular intervals

47
Q

How is the periodic table organised?

A

by increasing atomic number,

48
Q

Atomic radius definition

A

one-half the distance between the nuclei of identical atoms that are bonded together

49
Q

Ionic radius definition

A

the distance between the nucleus and the electron in the outermost level of the most common ion of an element.

50
Q

definition of ionisation energy

A

the amount of energy required to remove an electron from a neutral atom in gaseous form

equation X(g) —> X+(g) + e

51
Q

does ionisation energy increase or decrease down a group?

A
  • decreases as you go down a group as the distance from the nucleus increases and therefore there is more shielding and less hold on valence electrons
52
Q

does ionisation energy increase or decrease across a period?

A
  • increases
  • as the positive charge of the nucleus increases, more hold, harder to remove an electron. Dips are due to slight differences in sub-levels and orbitals
53
Q

Electronegativity definition

A

Electronegativity is the measure of the relative attraction an atom has for a shared pair of electrons in a covalent bond

54
Q

do metals have high or low electronegativities & why?

A
  • metals have tend to lose electrons, do not attract electrons and have low electronegativites
  • non metals tend to gain electrons, attract electrons and have high electronegativities
55
Q

does electronegativity increase or decrease across a period?

A

electronegativity increases as you go across a period as the core charge grows and valence electrons experience a greater attractive force

56
Q

electron affinity definition

A

the change in energy of a neutral gaseous atom when an electron is added to the atom to form a negative ion. It is the atom’s likelihood of gaining an electron

57
Q

trends for electron affinity

A

ncreases upward for the groups and from left to right across periodsof a periodic table because the electrons added to energy levels become closer to the nucleus, thus a stronger attraction between the nucleus and its electrons

58
Q

trends for electron affinity

A

increases upward for the groups and from left to right across periodsof a periodic table because the electrons added to energy levels become closer to the nucleus, thus a stronger attraction between the nucleus and its electrons

59
Q

The result of this reaction:

2NaCl + Br2 –>

A

no reaction

60
Q

group

A 
columns of periodic table
# of group gives number of valence electrons in outer shell
61
Q

period

A 
rows of the periodic table
# of period gives the number of occupied electron shells
62
Q

Chemical Properties are largely determined by…

A

the number of electrons in the outer shell

63
Q

Alkali metal properties

A
  • good conductors of electricity
  • low densities
  • grey shiny surface when cut with a knife
  • very reactive metals
  • form ionic compounds with non-metals
  • low ionization energies
  • reactivity increases down a group
  • react with water to produce H and metal OH
  • reactivity: Li
64
Q

As the electron is being added to a negative species…..

A

it is the second affinity as it is the second electron to be added

65
Q

What happens when Cl2 (aq), is added to an aqueous solution of potassium iodide, KI (aq)?

A

Iodide ions are displaced to produce aqueous iodine molecules
Cl2 (aq) + 2I− (aq) → 2Cl− (aq) + I2 (aq).

Chlorine is more reactive than iodine (it is a more powerful oxidising agent than iodine), therefore, it can displace iodide ions in solution.

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