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Chemistry > Trends in the Periodic table > Flashcards

Trends in the Periodic table Flashcards

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1
Q

What are groups

A

Groups are vertical column. Elements in the same group have the same number of electrons in their outer shell

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2
Q

what is a period

A

A period is a horizontal row. Elements in the have same number of shells

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3
Q

What is the atomic radius

A

Half the distance between the nuclei of two atoms of the same element that are joined together by a single covalent bond

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4
Q

What is nuclear charge

A

The force of attraction between the positive protons in the nucleus and the negative electrons in the outer shell.

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5
Q

Why does atomic radius… down the groups of the periodic table

A

Increases
As you do down a group, each elements has one more shell of electrons than the previous. The negative outer electrons get further away from the positive nucleus. Screening effect increases

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6
Q

What is the screening effect

Down a group

A

The increase in nuclear charge as you go down a group is lessened by a screening effect. The electrons in the inner shells screen the outer electrons from the positive charge in the nucleus

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7
Q

The atomic radius … across a period because

A

Decreases
There a increase in effective nuclear charge
No increase in screening effect

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8
Q

What results in increasing nuclear charge

A

Number of protons increase, number of shells stay the same so the increase in effective nuclear charge,so there is a greater attractive force on the outer electrons

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9
Q

What is First ionisation energy

A

The minimum energy required to completely remove the most loosely bound electron from a neutral gaseous atom in its ground state

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10
Q

Ionisation energy … down a group because of

A

Decreases
Increasing screening effect.
Increasing atomic radius

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11
Q

Ionisation energy … across a period because of

A

Increases
Increasing nuclear charge
Decreasing atomic radius

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12
Q

Why do some elements have higher first ionisation energy?

A

These elements would have full/ half full sublevels. Full or half filled sublevels give an atom extra stability so more energy is required to remove an electron

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13
Q

What is second Ionisation energy of a atom

A

The energy required to remove an electron from an ion with one positive charge in the gaseous state.

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14
Q

What is the formula for second ionisation energy

A

X+(g) —-> X2+(g) + e-
( small 2+)
X= element
g= state of matter

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15
Q

What is the first, second and third ionisation energy of potassium

A

K(g) —-> K+(g) + e-
K+(g) —> K2+ (g) + e-
K2+(g) —> K3+ (g) + e-

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16
Q

Why is there a large increase in ionisation energy whenever electrons are removed from a new sublevel or every level?

A

Decreased shielding effect

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17
Q

What is electronegativity

A

The relative attraction that an atom in a molecule has for the shared pair of electrons in a covalent bond

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18
Q

What happens to electronegativity when going down group and why

A

Electronegativity decreases going down a group.
1.increasing atomic radius
2. Increasing screening effect.

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19
Q

What happens to electronegativity values across a period

A

Electronegativity increases going across a period.
1 Increasing effective nuclear charge
2 Decreasing atomic radius

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20
Q

What do the chemical properties of an element depend on?

A

depends on their type of chemical bonding. How an element forms a bond is due to the number of electrons in the outer shell

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21
Q

Why are Alkali Metals reactive

A

They have a low ionization energy, the readily lose the single electron in their outer shell

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22
Q

Where are Alkali metals found

A

They are found in compounds, not free in nature itself

23
Q

Do the elements of group on lose their outer electrons easier or harder as you go down a group

A

Easier, because:
The atomic radius increases
Screening effect increases

24
Q

Reactions of Alkali metals with water

A

They all react vigorously with cold water.
Hydrogen gas is given off, metal hydroxide is produced
Speed and violence of the reaction increases as you go down a group- increased reactivity

25
Q

Describe the reaction of Lithium with water

A

Lithium floats, fizzes steadily and become smaller until it eventually disappears

26
Q

Describe the reaction of Sodium with water

A

The sodium melts to form a ball that moves around on the surface of the water. It fizzes rapidly, the hydrogen produced may produce a orange flame before the sodium disappears

27
Q

Word equation for reaction of Alkali metals with water

A

(element) + water —> (element) hydroxide + hydrogen

28
Q

Equation for reaction of Alkali metals with water

A

(element) + H2O —> (element)OH + 1/2 H2

29
Q

Reaction of alkali metals with Oxygen

A

When Alkali metals are cut they initially appear shiny grey but quickly become dull and white as they react with oxygen in the air- this is known as tarnishing

30
Q

How Lithium reacts with oxygen

A

Lithium tarnishes slowly due to its relatively slow reaction with oxygen

31
Q

How Sodium reacts with oxygen

A

Tarnishes quicker than lithium, its more reactive then Lithium

32
Q

How Potassium reacts with oxygen

A

Potassium tarnishes so quickly its difficult to see potassium is actually a shiny metal.

33
Q

Word equation for reaction of Alkali metals with oxygen

A

( element) + Oxygen –> (element) oxide

34
Q

Equation for reaction of Alkali metals with oxygen

A

2(element) + 1/2 O2 —> (element)2O

35
Q

In order for an atom to be stable what rule must it obey?

A

The octet rule, 8 electrons in the outer shell

36
Q

When a Halogen element reacts what does it do

A

It gains one electron

37
Q

Does the reactivity of halogens increase or decrease as you do down a group, and why?

A

Decreases,
The atomic radius increases
The effective nuclear charge decreases

38
Q

What can the reactivity of the halogens be shown by?

A

Displacement reactions

39
Q

Name and example of displacement reaction for the Halogens

A

When chlorine( as a gas or dissolved in water), is added to sodium bromide, the chlorine takes the place of the bromine. The chlorine is more reactive than bromine

40
Q

What’s the word formula for a displacement reaction of chlorine and bromine

A

Chlorine+ sodium bromide-> sodium chloride +bromide

41
Q

What do displacement reactions show.

A

A more reactive halogen displaced a less reactive halogen from a solution of one of its salts.the electronegativity decreases

42
Q

What is an Oxidising agent

A

A chemical which causes another chemical to lose an electron and become positivity charged

43
Q

what is a Redox reaction

A

One reactant has lost an electron and the other has gained an electron

44
Q

Redox reactions of the halogens

A

The halogens are very reactive elements, they are too unstable to exists in a nature in a uncombined form.They often react by taking an electron from another element, they act as oxidising agents. The smaller a halogen atom, the stronger oxidising agent it is.

45
Q

List the halogens in order of oxidising power

A

F >Cl >Br >I >At

46
Q

What is the colour of Chlorine in water

A

Pale green

47
Q

What is the colour of Bromine in water

A

Yellow/ orange

48
Q

What is the colour of Iodine in water

A

Brown/red

49
Q

What is the colour of Chloride ions in water

A

Colourless

50
Q

What is the colour of Bromide ions in water

A

Colourless

51
Q

What is the colour of Iodide ions in water

A

Colourless

52
Q

What is a diatomic molecule

A

A molecule that is made up of two atoms of the same or different elements

53
Q

What does AQ stand for in refrence to the state?

A

aqueous solution

54
Q

What does the acronym OIL RIG stand for

A

Oxidation Is Loss, Reduction Is Gain

Chemistry (27 decks)

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