Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry Paper 1 > C2 - The Periodic Table > Flashcards

C2 - The Periodic Table Flashcards

(46 cards)

Start Studying
1
Q

What is the periodic table?

A

A list of elements arranged according to their atomic number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

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

A

The noble gases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What determines an element’s chemical properties?

A

The number of electrons in its outer shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

List three general physical properties of metals.

A
  • Lustrous (shiny)
  • Good conductor
  • Malleable and ductile
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

List three general physical properties of non-metals.

A
  • Dull
  • Poor conductor
  • Brittle
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Where are metals located on the periodic table?

A

On the left side

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Where are non-metals located on the periodic table?

A

On the right side

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What type of ions do metals form?

A

Positive ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What type of ions do non-metals form?

A

Negative ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What does the group number in the periodic table indicate?

A

How many electrons are in the element’s outer shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What does the period number in the periodic table indicate?

A

How many shells of electrons an element has

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

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

A

Mendeleev and Newlands

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What was Newlands’ Law of Octaves?

A

Every 8th element had similar properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What criticism did Newlands face regarding his periodic table?

A

He grouped elements with very different properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

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

A

False

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

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

20
Q

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

21
Q

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

Study These Flashcards
A

He left gaps for undiscovered elements

22
Q

Which two scientists are credited with early periodic table proposals?

Study These Flashcards
A

Mendeleev and Newlands

23
Q

List two properties of metals.

Study These Flashcards
A
  • High melting point
  • Strong
24
Q

List two properties of non-metals.

Study These Flashcards
A
  • Low melting point
  • Low density
25
What are Group 7 elements commonly known as?
Halogens ## Footnote Halogens include fluorine, chlorine, bromine, and others.
26
How many electrons are in the outer shell of Group 7 elements?
Seven ## Footnote This configuration influences their chemical behavior.
27
What type of molecules do halogens exist as?
Diatomic molecules ## Footnote Examples include F2, Cl2, Br2.
28
What happens when a more reactive halogen is introduced to a compound?
It can displace another halogen ## Footnote Example: potassium bromide + chlorine → potassium chloride + bromine.
29
What trend occurs in the density, boiling point, and melting point of halogens as you move down the group?
They increase ## Footnote Reactivity decreases down the group.
30
What are Group 0 elements also known as?
Noble Gases ## Footnote These include helium, neon, argon, and others.
31
Why are noble gases considered unreactive?
They have a complete outer shell of electrons ## Footnote This stability prevents them from reacting easily.
32
What happens to the boiling points of noble gases as you move down the group?
They increase ## Footnote This trend is consistent across the group.
33
What are Group 1 metals commonly referred to as?
Alkali Metals ## Footnote They produce alkaline solutions when reacting with water.
34
What is the characteristic of Group 1 elements related to their outer shell?
They have a single electron ## Footnote This leads them to lose an electron to achieve stability.
35
What trend occurs in the density and reactivity of Group 1 metals as you move down the group?
They increase ## Footnote Melting point decreases down the group.
36
What do Group 1 elements react vigorously with to form chlorides?
Chlorine ## Footnote Example: sodium + chlorine → sodium chloride.
37
What do Group 1 metals form when they react with oxygen?
Metal oxides ## Footnote Example: potassium + oxygen → potassium oxide.
38
What do Group 1 metals produce when they react with water?
Metal hydroxide and hydrogen ## Footnote Example: sodium + water → sodium hydroxide + hydrogen.
39
Where are transition metals located in the periodic table?
Central section ## Footnote Includes elements like chromium (Cr), cobalt (Co), and iron (Fe).
40
How do transition metals generally compare to Group 1 metals in terms of physical properties?
Harder, stronger, denser, higher melting points ## Footnote Transition metals are typically more robust.
41
Are transition metals more or less reactive than Group 1 metals?
Less reactive ## Footnote Some transition metals do not react with oxygen or water at all.
42
What role do transition metals commonly serve in chemical processes?
Catalysts ## Footnote They facilitate reactions without being consumed.
43
What is the relationship between reactivity and the ability to lose or gain electrons?
More easily an electron is lost or gained, the more reactive the element ## Footnote This principle applies to both metals and non-metals.
44
How does the reactivity of Group 1 elements change as you move down the group?
Increases ## Footnote This is due to larger atomic size and weaker attraction to the nucleus.
45
How does the reactivity of Group 7 elements change as you move down the group?
Decreases ## Footnote Larger atomic size makes it harder to gain an electron.
46
What is an example of an element that can form ions with different charges?
Iron ## Footnote It can form Fe²⁺ and Fe³⁺ ions.

Chemistry Paper 1 (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions