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Chem HL > The periodic table > Flashcards

The periodic table Flashcards

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1
Q

What are some properties of group 1 Alkali metals

A

Soft
Highly reactive
Low melting points
Form soluble salts

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2
Q

Where are the d - block elements

A

3-12

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3
Q

What are non - metal properties

A

poor conductors
not hard
solid , liquid or gas at room temperature

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4
Q

At room temperature what are florine and chlorine

A

Gasses

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5
Q

At room temperature what is Br

A

liquid

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6
Q

At room temperature what is I

A

solid

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7
Q

What are the properties of the Noble gasses

A

Highly reactive
Gases

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8
Q

What is the first row of the f-block called

A

Lanthanides

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9
Q

What is the second row of the f-block called

A

Actinides

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10
Q

What are the properties of f-block

A

Complex and heavy metals
Highly reactive
High melting and boiling points

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11
Q

Elements in the same period have the same number of

A

shells

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12
Q

Across a period
Charge of nucleus …
Atomic Radius …

A

Increases
Decreases

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13
Q

Where are the metals and non-metals located

A

metals - left
non metals - right

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14
Q

Definition of Ionisation Energy

A

The energy needed to remove one mol of an electron from a mole of gaseous atoms of ions

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15
Q

Atomic radius and Ionisation Energy are

A

Inversely Proportional

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16
Q

What happens down a group between
Atomic radius :
Ionisation Energy :

A

Increases
Decrease

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17
Q

What happens across a period between
Atomic Radius
Ionisation Energy

A

Decrease
Increase

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18
Q

Define electron affinity

A

The energy released when one mole of an atom gains an electron to form a negatively charged ion

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19
Q

Explain the trend between electron affinity down the group

A

decreases

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20
Q

Explain the trend between electron affinity across a period

A

increases

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21
Q

Define Electronegativity

A

The ability of an atom to attract a pair of bonded electrons

22
Q

Electronegativity decreases down a group because

A

nuclear charge increases
increased shielding
large atomic radius due to increase in electron shell

23
Q

Electronegativity increased across a period because

A

Effective nuclear charge increases
Stronger attraction between the nucleus and the shared pair of electrons

24
Q

What decreases as you go down group 1

A

ionisation energy

25
Q

What increases as you go down group 1

A

reactivity
number of occupied energy levels

26
Q

What increases down group 17

A

number of occupied energy levels

27
Q

What decreases down group 17

A

electron affinity
reactivity

28
Q

Define first ionisation energy

A

minimum energy required to lose one mole of electrons from one mole of gaseous atoms to produce one mole of gaseous ions

29
Q

Explain why the first ionisation energy decreases down a group (3)

A

• Going down a group atomic radii increases and electrons occupy higher energy levels
• Electrons in higher energy levels have a weaker attraction to the nucleus.
• Less energy is required in order to remove an electron

30
Q

Explain why first ionisation energy increases across a period

A

Going across there are more protons in the nucleus and more electrons occupying the outermost energy level (effective nuclear charge)

• A greater number of electrons in the outermost energy level results in a stronger attraction to the nucleus

• More energy is required in order to remove an electron

31
Q

Atomic radius

A

Increases down a group
decreases across a period

32
Q

Define First Electron affinity

A

the amount of energy released when a neutral atom gains an electron to form a negatively charged ion

33
Q

Why does First electron affinity decrease down a group

A

The atomic radius becomes larger , the attraction for an additional electron is less , since the effective nuclear charge is reduce due to increased shielding

34
Q

Why does electron affinity increase across a period

A

Elements across a period have a higher effective nuclear charge.
Stronger attraction between the added electron and the nucleus

35
Q

What are the 6 characteristic properties of transition elements

A

• Variable oxidation states
• High melting points
• Magnetic properties
• Catalytic properties
• Formation of coloured compounds
• Formation of complex ions

36
Q

if the ionisation number is 2+ what its oxidation number

A

+2

37
Q

What is a transition element

A

element with a partially filled d-subshell

38
Q

what is effective nuclear charge

A

more electrons in shells

39
Q

What type of metals have low EA

A

metals

40
Q

What type of metals have a high EA

A

non-metals

41
Q

Why do metals have low electronegativities

A

because they lose electrons easily

42
Q

why do non-metals have high electronegativities

A

as they gain electrons to fill their outer shell

43
Q

What is the trend in melting points ?

A

Increase across a period until group 14 then decrease

44
Q

What is the trend in metallic character

A

Increases down a group
Decreases across a period

45
Q

What is the acidic state of sodium oxide Na2O

A

Basic

46
Q

What is the acidic state of magnesium oxide Mgo

A

Basic

47
Q

What is the acidic state of Aluminium Oxide Al2O3

A

Amphoteric

48
Q

What is the acidic state of Silicon Oxide SiO2

A

acidic

49
Q

What is the acidic state of Phosphorus

A

Acidic

50
Q

What is the acidic state of sulfur oxide SO2

A

acidic

51
Q

What is the acidic state of chlorine oxide

A

Acidic

Chem HL (13 decks)

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