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Periodic Table Flashcards

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1
Q

Why were early versions of the periodic table incorrect?

A

They were arranged in order of increasing atomic weight but they were unaware of isotopes. Therefore some elements were placed in the wrong order.

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2
Q

How did Mendeleev structure his periodic table?

A

He ordered the elements based on atomic weight, but also lined up elements with similar properties in the same column.

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3
Q

Why did Mendeleev leave gaps in his periodic table?

A

He left spaces for elements he believed had not yet been discovered.

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4
Q

How are elements in the periodic table arranged?

A

By atomic number (number of protons in nucleus).

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5
Q

What are the vertical columns on the periodic table called?

A

Groups.

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6
Q

How are elements in the same group similar?

A

They have the same number of electrons in their outer shell which gives them similar chemical properties.

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7
Q

What are the horizontal rows on the periodic table called?

A

Periods.

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8
Q

How are elements in the same period similar?

A

They have the same number of electron shells.

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9
Q

What are the five main properties of a metal?

A
  • They are shiny (good reflectors of light)
  • Good conductors of heat (transfer energy through the heating pathway effectively)
  • Good conductors of electricity (we use them to make wires for circuits)
  • Strong (can withstand large forces)
  • Malleable (can bend without breaking, which allows them to be shaped)
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10
Q

What happens to metals when they react with other elements?

A

They lose electrons from their outer shells to form full outer shell, which makes them overall positively charged (a cation).

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11
Q

What do non-metal atoms form?

A

An anion.

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12
Q

What is group 0?

A

Noble gases.

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13
Q

Why are noble gases inert (unreactive)?

A

They have full outer shells.

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14
Q

Why is helium used in weather balloons and airships?

A

It is less dense than air, so it enables them to float.

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15
Q

Why is hydrogen not used in weather balloons and airships?

A

Although, like helium, it is less dense than air, it is flammable so it will react with the oxygen in the air and catch fire.

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16
Q

What is argon used for?

A

It is denser than air so it is put in the space above the wine in a wine bottle to prevent the wine from reacting with air.

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17
Q

What happens as you go down group 0 in the periodic table? (D Mp Bp Am)

A
  • Density increases
  • Melting point increases
  • Boiling point increases
  • Atomic mass increases
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18
Q

What is group 1 in the periodic table?

A

Alkali metals.

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19
Q

Why are alkali metals highly reactive?

A

They only have one electron in their outer shell to lose and become more stable.

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20
Q

What do metals form with non-metals?

A

Ionic compounds formed between positive and negative ions.

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21
Q

What are ionic compounds held together by?

A

Electrostatic force.

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22
Q

Why does reactivity increase as you go down group 1?

A
  • The atoms increase in size
  • This means that the distance between the positive nucleus and negative electrons increases because there are more electron shells
  • This means that the force holding the electrons in orbit becomes weaker, so electrons are lost more easily
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23
Q

What are the metals towards the bottom of group 1 like?

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A

Extremely reactive and dangerous.

24
Q

What are the three main properties of alkali metals?

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A
  • Soft
  • Can be easily cut
  • Have low melting points
25
What happens to alkali metals as you go down the group? (R Am Mp Bp)
- Reactivity increases - Atomic mass increases - Melting point decreases - Boiling point decreases
26
What does an equation look like when you react an alkali metal with water?
Alkali metal + Water -> Metal hydroxide + Hydrogen
27
What does an equation look like when you react an alkali metal with chlorine?
Alkali metal + Chlorine -> Metal chloride
28
What does an equation look like when you react an alkali metal with oxygen?
Alkali metal + Oxygen -> Metal oxide
29
What does the alkali metal and chlorine look like before the reaction?
Grey solid metal and green smoke
30
What does the alkali metal and chlorine look like during the reaction?
White smoke and a coloured flame
31
What does the alkali metal and chlorine look like after the reaction?
Solid powder
32
What is group 7?
The Halogens
33
Are Halogens metals or non-metals?
Non-metals
34
What do Halogens form?
Molecules consisting of pairs of atoms that are covalently bonded
35
How many electrons do Halogens have in their outer shells?
7
36
Why do halogens attract electrons?
To form full outer shells and become stable.
37
What happens when halogens gain full outer shells?
They become negatively charged with a charge of -1 as they gain an electron.
38
What happens to the number of shells as you progress down group 7?
There's more of them. This increases the distance between the nucleus and outer shell.
39
What happens as the distance between a nucleus and it's outer shell increases?
- The nucleus is positively charged (protons) - The positive charge attracts the missing electron from it's outer shell - As distance increases, the shielding effect of the extra shell increases - The force attracting the missing electron gets weaker
40
What decreases as you go down group 7? (R)
Reactivity
41
Why are smaller halogens more reactive?
- The positive nucleus is closer to the outer electron shell - The force of attraction of electrons is greater - The reactivity decreases as you go down the group
42
What increases as you go down group 7? (R, M, B)
- Relative atomic mass - Melting point - Boiling point
43
What is formed when a metal and a halogen react and why?
- A salt - An electron has left the metal (cation) - An electron has joined the halogen (anion) - Opposite charges attract (ionic bond)
44
What can more reactive halogens do?
- Displace a less reactive halogen - This forms a salt dissolved in water
45
What properties do hard metals have?
- Difficult to scratch - Difficult to dent - Difficult to cut
46
What properties do soft metals have?
- Scratch easily - Dent easily - Cut easily
47
Where are transition metals located on the Periodic Table?
The centre.
48
What are the two main similarities between transition metals and alkali metals?
- Conduct electricity - Shiny when cut
49
Typically, which has the higher melting point, transition metals or alkali metals?
- Transition metals have very high melting points (1400C-2000C) - Alkali metals have lower melting points (<200C)
50
Typically, which has the higher density, transition metals or alkali metals?
- Alkali metals are less dense (float on water) - Transition metals are more dense (sink in water)
51
Typically, which is harder, transition metals or alkali metals?
- Alkali metals are softer (can be cut with scalpel) - Transition metals are harder (need special equipment)
52
Typically, which has the higher strength, transition metals or alkali metals?
- Alkali metals are weaker (easily broken in half) - Transition metals are stronger (used to construct buildings and bridges)
53
Typically, which is more reactive, transition metals or alkali metals?
- Alkali metals are more reactive (with water, oxygen and halogens) - Transition metals are less reactive
54
How do alkali metals react with oxygen (room temp), cold water and halogens?
Vigorously
55
How do transition metals react with oxygen (room temp), cold water and halogens?
- Slowly or not at all - Slowly or not at all - A few will react with the halogens

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