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Chemistry IGCSE > Unit 8 - The Periodic Table > Flashcards

Unit 8 - The Periodic Table Flashcards

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1
Q

Arrangement of elements in the periodic table

A

Arranged by atomic number

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2
Q

Amount of elements in the periodic table

A

118 - 94 occur naturally

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3
Q

Groups

A

The columns of the periodic table

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4
Q

Periods

A

The rows of the periodic table

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5
Q

Number of groups in the periodic table

A

8

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6
Q

Features of elements on the periodic table

A

Nucleon number and proton number

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7
Q

Properties of metals in the periodic table

A
  • Large atomic radius
  • Conduct heat and electricity
  • Have a range of melting point values
  • Malleable and ductile
  • Shiny
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8
Q

Properties of non-metals in the periodic table

A
  • Smaller atomic radius
  • Do not conduct heat or electricity
  • Generally low melting point values
  • Brittle
  • Dull
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9
Q

Metalloids

A

Elements that display properties of both metals and non-metals - found in the middle of the periodic table

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10
Q

Trends in groups of the periodic table

A

All elements in the same group have the same number of electrons in their outer shell

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11
Q

Relationship with have the same number of electrons on the outer shell

A

Elements with the same number of outer shell electrons react similarly

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12
Q

Period number relationship in the periodic table

A

The period number shows how many shells an element has

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13
Q

Group number relationship in the periodic table

A

The group number shows how many electrons are on the outer shell of the elements

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14
Q

Metal atoms relationship with ions

A

Metal atoms lose electrons and form positively charged ions

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15
Q

Non-metal atoms relationship with ions

A

Non-metal atoms gain electrons to form negatively charged ions

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16
Q

Groups and ion charges

A
  • Group 1 = 1+
  • Group 2 = 2+
  • Group 3 = 3+
  • Group 4 = N/A
  • Group 5 = 3-
  • Group 6 = 2-
  • Group 7 = 1-
  • Group 8 = 0
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17
Q

Covalent radius

A

Measure of how large individual atoms are

18
Q

Relationship with covalent radius and the periodic table

A
  • Increases as you go down a group
  • Decreases as you go across a period
19
Q

Group 1 metals name

A

The alkali metals

20
Q

Elements in group 1

A

Lithium, Sodium, Potassium, Rubidium, Caesium, Francium

21
Q

Chemical properties of Group 1 metals

A
  • Reactivity increases down the group
  • Density increases down the group
  • Melting point decreases down the group
  • Reacts more vigorously with water down the group
22
Q

Lithium and water reaction

A
  • Happens on the surface of the water
  • Hydrogen gas given off
  • Effervescence can be seen
  • Lithium moves around on the surface
  • Water will become alkaline
23
Q

Lithium + water equation

A
  • Lithium + Water –> Lithium hydroxide + Hydrogen
  • 2Na(s) + 2H2O(l) –> 2NaOH(aq) + H2(g)
24
Q

Sodium and water reaction

A
  • Reaction is more vigorous than Lithium
  • Heat given off
  • Metal moves on the surface of the water faster
25
Q

Sodium + water equation

A
  • Sodium + water –> Sodium hydroxide + hydrogen
  • 2Na(s) + 2H2O(l) –> 2NaOH(aq) + H2(g)
26
Q

Potassium and water reaction

A
  • Enough heat to ignite the hydrogen gas
  • Lilac flame
  • Potassium hops around the surface of the water
27
Q

Potassium + water equation

A
  • Potassium + Water –> Potassium hydroxide + Hydrogen
  • 2K(s) + 2H2O(l) –> 2KOH(aq) + H2(g)
28
Q

Reason for increasing reactivity

A

More shells leads to a higher atomic radius, losing less traction with the nucleus and causing the electron to be easier to lose

29
Q

Name of Group VII elements

A

The Halogens

30
Q

Features of halogens

A
  • Non-metals
  • Diatomic molecules
31
Q

Colors of elements in Group VII

A
  • Chlorine - Yellow-green gas
  • Bromine - Red-Brown liquid
  • Iodine - Dark purple solid
  • Increasing darkness
32
Q

Trends of The Halogens down the group

A
  • Increasing darkness
  • Increasing density
  • Melting point increases
  • Reactivity decreases
33
Q

Reasons for decreasing reactivity

A

The ability to attract an extra electron on more outer shells weakens

34
Q

Features of transition elements

A
  • High densities
  • High melting points - except for Mercury
  • Not very reactive
  • Don’t react rapidly with air or water
  • very stable
  • Form colored compounds
  • Variable oxidation numbers
35
Q

Uses of transition metals

A
  • Jewelry
  • catalysts e.g. iron to make ammonia
36
Q

Variable oxidation state

A

An element can form different ions by losing a different number of electrons e..g Iron(II) or Iron(III)

37
Q

Name for group VIII elements

A

The noble gases

38
Q

Noble Gases

A

Helium, Neon, Argon, Krypton, Xenon, Radon, Oganesson

39
Q

Features of noble gases

A
  • Colorless gases
  • Monatomic
  • Complete outer shells
  • Inert - not reactive
40
Q

Trends of noble gases down the group

A
  • Boiling point decreases
  • Density increases

Chemistry IGCSE (12 decks)

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