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C4.1-C4.2 > Recall the physical and chemical properties of groups 1, 7 & 0 > Flashcards

Recall the physical and chemical properties of groups 1, 7 & 0 Flashcards

1
Q

What are group 1 metals known as

A

The alkali metals

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2
Q

Why do alkali metals all have similar chemical properties

A
  • They all have one electron in the outer shell
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3
Q

What are the physical properties of alkali metals

A
  • Low melting and boiling points compared to other metals
  • low density - Li, Na, K float on water
  • Very soft - they can be cut with a knife
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4
Q

Why are group 1 metals reactive?

A
  • They readily lose their one outer electron to form a +1 ion to get a stable electronic structure
  • as you go down group 1 the alkali metals get more reactive
  • because outer electron is easily lost because the atomic radius is larger
  • therefore it’s less strongly attracted to nucleus and less energy needed to remove it
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5
Q

Describe the reaction between a alkali metal and cold water

A
  • Reacts vigorously
  • produces metal hydroxide + hydrogen
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6
Q

describe the reaction between rubidium and cesium with water

A
  • react violently with watee and explode
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7
Q

what is the balanced equation of sodium + water

A

2Na+2H2O→2NaOH+H2

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8
Q

What are the group trends for group 1

A

Down the group:

  • increasing atomic radius
  • decreasing electronegativity
  • increasing reactivity
  • decreasing melting and boiling pointsincreasing atomic radius
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9
Q

What would you see when lithium reacts with water

A
  • When lithium is added to wafter it floats.
  • It fizzes steadily and becomes smaller, until it eventually disappears.
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10
Q

What is the word and symbol equation for lithium reacting with water

A
  • lithium + water → lithium hydroxide + hydrogen
  • 2Li(s) + 2H2O(l) → 2LiOH(aq) + H2(g)
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11
Q

What would you see if sodium reacted with water

A
  • the sodium melts to form a ball that moves around on the surface
  • It fizzes rapidly
  • produces hydrogen that may burn with an orange flame before the sodium disappears.
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12
Q

What is the word and symbol equation of sodium reacting with water

A
  • sodium + water → sodium hydroxide + hydrogen
  • 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
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13
Q

What would you see if potassium reacted with water

A

When potassium is added to water

  • It melts and floats around very quickly on the surface of the water.
  • The hydrogen ignites instantly.
  • The metal is also set on fire, with sparks and a lilac flame.
  • There is sometimes a small explosion at the end of the reaction.
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14
Q

What is the word and symbol equation for potassium reacting with water

A
  • potassium + water → potassium hydroxide + hydrogen
  • 2K(s) + 2H2O(l) → 2KOH(aq) + H2(g)
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15
Q

what are group 7 elements known as?

A

the halogens

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16
Q

what are the elements on group 7

A
  • fluorine
  • chlorine
  • bromine
  • iodine
  • astatine
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17
Q

why do group 7 elements exist as diatomic molecules?

A

because they share a pair of electrons in a covalent bond giving both toms a full outer shell

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18
Q

what happens as you go down group seven ?

A
  • melting and boiling points increase
  • reactivity decreases
  • Color becomes darker
  • State of change gas to liquid to solid
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19
Q

at room temperature what color is

  1. chlorine
  2. bromine
  3. iodine
A
  • chlorine: fairly reactive, poisonous green gas
  • bromine: poisonous brown orange liquids gives off an orange vapor at room temp
  • iodine: dark grey solid purple vapor when heated
20
Q

why does reactivity decrease going down group 7

A
  • gain one electron to 1- ion
  • as you go down the group, less reactive as it gets harder to gain extra electron to make full outer shell when its further away form the nucleuas
21
Q

what happens when halogens react with alkali metals

A
  • form salts called metal halides
  • eg : sodium+ chlorine → sodium chloride | 2Na+Cl2 → 2NaCl
  • eg: potassium + bromine → potassium bromide | 2K+Br2→ 2KBr
22
Q

what is a displacement reaction?

A
  • a displacement reaction is where a more reactive element displaces a less reactive element from a compound
23
Q

describe what happens in the chlorine water and potassium bromide practical

A
  • chlorine is more reactive than bromine
  • if you add chlorine water to potassium bromide
  • chlorine will displace the bromine and becomes potassium chloride
  • the bromide ions are oxidized to bromine turning orange
24
Q

write a balanced equation for chlorine and potassium bromide displacement reaction

A

chlorine + sodium bromide → sodium chloride + bromine

Cl2(aq) + 2NaBr(aq) → 2NaCl(aq) + Br2(aq)

25
Q

how can displacement reactions show reactivity trends

A
  • start by adding small amount of halide solution in test tube
  • add a few drops of a halogen solution to it and shake tube gently
  • color change=reaction
  • the halogen replaced the halide ions from salt
  • no color change no reaction
26
Q

explain what is happening and what is made

A

when chlorine water is added to:

  • potassium bromide solution-an orange solution is formed
  • potassium iodide solution - a brown solution is formed

when bromine water is added to:

  • potassium iodide solution- a brown solution is formed
  • chlorine displaces both bromine and iodine . bromine only displaces iodine . Iodine doesn’t displace either
27
Q

Florine reaction with iron wool

A
  • Reacts with almost anything instantly.
  • dangerous
28
Q

Chlorine reaction with iron wool

A

Reacts with heated iron wool very quickly.

29
Q

Bromine reaction with iron wool

A

Has to be warmed and the iron wool heated. The reaction is faster.

30
Q

Iodine reaction with iron wool

A

Has to be heated strongly and so does the iron wool. The reaction is slow

31
Q

Why do boiling and melting points increase as you go doen group 7

A
  • the molecules become larger
  • the intermolecular forces become stronger
  • more energy is needed to overcome these forces
32
Q

What is made when a halogen reacts with a non metal

use chlorine and hydrogen

A
  • A compound is formed
  • hydrogen + chlorine → hydrogen chloride
  • H2(g) + Cl2(g) → 2HCl(g)
33
Q

Describe the reaction between hydrogen and Florine

A
  • Explodes at room temperature and in the dark, forming hydrogen fluoride
34
Q

Describe the reaction between hydrogen and chlorine

A

Explodes with a flame or in sunlight, forming hydrogen chloride

35
Q

Describe the reaction between hydrogen and bromine

A
  • Vigorous reaction when warmed with hydrogen, forming hydrogen bromide
36
Q

Describe the reaction between hydrogen and iodine

A
  • Very slow reaction when heated strongly, forming some hydrogen iodide
37
Q

What happens when the hydrogen halides are put into water

A

The hydrogen halides are gases at room temperature. They dissolve** in water to produce **acidic** **solutions.

38
Q

what is group zero known as

A
  • the noble gasses
39
Q

at room temperature what color are all of the gasses ?

A

colorless

40
Q

why are the noble gasses all monotonic

A
  • because they’re all made up of single atoms
41
Q

why are the noble gasses inert (unreactive)

A
  • because they all have full outer shells
  • meaning they dont give or gain electrons easily
42
Q

why are the noble gasses non flammable

A

because they are inert

43
Q

name the group zero elements

A
  • helium
  • neon
  • argon
  • krypton
  • xenon
  • radon
44
Q

as you go down the group what happens to the

  • boiling point
  • melting point
  • density
A

increase

45
Q

how to estimate the densities of group 0 elements

eg use the densities of helium (0.2kg/m3) and argon (1.8kg/m2) to estimate the density of neon

A
  • (0.2 + 1.8)/2=1
  • neon should have a density around 1kg/m3
46
Q

why do group 0 elements react in similar ways

A
  • they all have full outer electron shells

C4.1-C4.2 (3 decks)

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