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Chemistry Paper 1 > C2 - The Periodic Table > Flashcards

C2 - The Periodic Table Flashcards

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1
Q

What is the periodic table?

A

A list of elements arranged according to their atomic number

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2
Q

What do elements in the same group of the periodic table have in common?

A

The same number of electrons in their outer shell and similar properties

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3
Q

Which group of elements is known for being very unreactive gases?

A

The noble gases

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4
Q

What determines an element’s chemical properties?

A

The number of electrons in its outer shell

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5
Q

List three general physical properties of metals.

A
  • Lustrous (shiny)
  • Good conductor
  • Malleable and ductile
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6
Q

List three general physical properties of non-metals.

A
  • Dull
  • Poor conductor
  • Brittle
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7
Q

Where are metals located on the periodic table?

A

On the left side

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8
Q

Where are non-metals located on the periodic table?

A

On the right side

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9
Q

What type of ions do metals form?

A

Positive ions

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10
Q

What type of ions do non-metals form?

A

Negative ions

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11
Q

What does the group number in the periodic table indicate?

A

How many electrons are in the element’s outer shell

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12
Q

What does the period number in the periodic table indicate?

A

How many shells of electrons an element has

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13
Q

Who proposed an early version of the periodic table based on atomic weight?

A

Mendeleev and Newlands

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14
Q

What was Newlands’ Law of Octaves?

A

Every 8th element had similar properties

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15
Q

What criticism did Newlands face regarding his periodic table?

A

He grouped elements with very different properties

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16
Q

What was a significant change in the arrangement of the modern periodic table?

A

It is arranged by atomic number instead of atomic weight

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17
Q

How did the discovery of isotopes impact the periodic table?

A

It explained why ordering elements by atomic weight was not always correct

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18
Q

True or False: All elements in the same group have the same number of protons.

A

False

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19
Q

Fill in the blank: The elements with atomic numbers 58 - 71 are called the _______.

A

Lanthanides

20
Q

Fill in the blank: The elements with atomic numbers 90 - 103 are called the _______.

A

Actinides

21
Q

What was one of the key contributions of Mendeleev to the periodic table?

A

He left gaps for undiscovered elements

22
Q

Which two scientists are credited with early periodic table proposals?

A

Mendeleev and Newlands

23
Q

List two properties of metals.

A
  • High melting point
  • Strong
24
Q

List two properties of non-metals.

A
  • Low melting point
  • Low density
25
Q

What are Group 7 elements commonly known as?

A

Halogens

Halogens include fluorine, chlorine, bromine, and others.

26
Q

How many electrons are in the outer shell of Group 7 elements?

A

Seven

This configuration influences their chemical behavior.

27
Q

What type of molecules do halogens exist as?

A

Diatomic molecules

Examples include F2, Cl2, Br2.

28
Q

What happens when a more reactive halogen is introduced to a compound?

A

It can displace another halogen

Example: potassium bromide + chlorine → potassium chloride + bromine.

29
Q

What trend occurs in the density, boiling point, and melting point of halogens as you move down the group?

A

They increase

Reactivity decreases down the group.

30
Q

What are Group 0 elements also known as?

A

Noble Gases

These include helium, neon, argon, and others.

31
Q

Why are noble gases considered unreactive?

A

They have a complete outer shell of electrons

This stability prevents them from reacting easily.

32
Q

What happens to the boiling points of noble gases as you move down the group?

A

They increase

This trend is consistent across the group.

33
Q

What are Group 1 metals commonly referred to as?

A

Alkali Metals

They produce alkaline solutions when reacting with water.

34
Q

What is the characteristic of Group 1 elements related to their outer shell?

A

They have a single electron

This leads them to lose an electron to achieve stability.

35
Q

What trend occurs in the density and reactivity of Group 1 metals as you move down the group?

A

They increase

Melting point decreases down the group.

36
Q

What do Group 1 elements react vigorously with to form chlorides?

A

Chlorine

Example: sodium + chlorine → sodium chloride.

37
Q

What do Group 1 metals form when they react with oxygen?

A

Metal oxides

Example: potassium + oxygen → potassium oxide.

38
Q

What do Group 1 metals produce when they react with water?

A

Metal hydroxide and hydrogen

Example: sodium + water → sodium hydroxide + hydrogen.

39
Q

Where are transition metals located in the periodic table?

A

Central section

Includes elements like chromium (Cr), cobalt (Co), and iron (Fe).

40
Q

How do transition metals generally compare to Group 1 metals in terms of physical properties?

A

Harder, stronger, denser, higher melting points

Transition metals are typically more robust.

41
Q

Are transition metals more or less reactive than Group 1 metals?

A

Less reactive

Some transition metals do not react with oxygen or water at all.

42
Q

What role do transition metals commonly serve in chemical processes?

A

Catalysts

They facilitate reactions without being consumed.

43
Q

What is the relationship between reactivity and the ability to lose or gain electrons?

A

More easily an electron is lost or gained, the more reactive the element

This principle applies to both metals and non-metals.

44
Q

How does the reactivity of Group 1 elements change as you move down the group?

A

Increases

This is due to larger atomic size and weaker attraction to the nucleus.

45
Q

How does the reactivity of Group 7 elements change as you move down the group?

A

Decreases

Larger atomic size makes it harder to gain an electron.

46
Q

What is an example of an element that can form ions with different charges?

A

Iron

It can form Fe²⁺ and Fe³⁺ ions.

Chemistry Paper 1 (7 decks)

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