Periodic Table Flashcards

1
Q

What changes when moving top to bottom down the periodic table?

A
  • Proton number increases not consecutively
  • Number of electron shells increases consecutively
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
1
Q

What changes when we move left to right across the periodic table?

A
  • Proton Number increases consecutively
  • Number of valence electrons increases consecutively
  • Different chemical properties
  • Elements change from metals to non-metals
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

How does reactivity change when going down group 1 (alkali metals)

A

Reactivity increases

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

State physical properties of alkali metals.

A
  • Lower melting points and boiling points compared to other metals
  • Lower density compared to other metals
  • Soft (Able to cut easily)
  • Shiny silvery solids
  • Conducts Electricity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

State the chemical properties of alkali metals.

A
  • Strong alkalis
  • turns colour of universal indicator green to violet
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

State the observations made when sodium reacts with water.

A
  • Sodium dart around the surface of water (less dense than water)
  • Fizzing/Effervescence can be observed
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

State the trends going down group 1

A
  • Melting Point Decreases
  • Reactivity increases
  • Density increases (except potassium)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Why does reactivity of alkali metals increasing going down the group.

A

Atomic size of elements increase, Increase in number of electron shells. → Attraction between positively charged nucleus and valence electrons decreases as valence electrons are further away from the nucleus. → Easier to lose the valence electron going down the group.

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

How does reactivity change when going down group 17?

A

Reactivity decreases

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

State physical properties of Halogens

A
  • Low melting and boiling points
  • are coloured elements
  • cannot conduct electricity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Colour and state of flourine in r.t.p

A
  • Pale yellow
  • Gas
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Colour and state of chlorine in r.t.p

A
  • Greenish-Yellow
  • gas
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Colour and state of Bromine in r.t.p

A
  • Reddish Brown
  • Liquid
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Colour and state of Iodine in r.t.p

A
  • Purple Black (Brown Solution)
  • Solid
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Colour and state of Astatine in r.t.p

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

Why does reactivity decreases down group 17?

A

Atomic size of elements increase, Increase in number of electron shells. → Attraction between positively charged nucleus and valence electrons decreases as valence electrons are further away from the nucleus. → More difficult to gain an electron to obtain a stable noble gas configuration

16
Q

Why does m.p and b.p increases down group 17?

A

Group 17 elements are a covalent substance and exists as simple discrete molecules.→ As the mass of halogens increases down the group, the intermolecular forces of attraction are strengthened. → More energy is needed to overcome the stronger intermolecular forces of attraction down the group. → Going down the group, elements change from gas to liquid then to solid

17
Q

What are the similarities between hydrogen and alkali metals?

A
  • Atoms of these elements lose 1 electron to form positive ion of 1+ charge.
  • Atoms of these elements have one valence electron.
18
Q

What are the differences between hydrogen and alkali metals?

A
  • Atoms of hydrogen can gain electron to form anion (H−) whereas atoms of Group 1 lose electron to form cation.
  • Hydrogen exists as a gas whereas Group 1 elements exist as solid state at room temperature and pressure.
  • Hydrogen does not conduct electricity whereas Group 1 elements conduct electricity well.
  • Hydrogen is colourless gas, Group 1 are shiny and silvery solids.