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chemistry (paper one) > groups 1,7,0 (topic 1) > Flashcards

groups 1,7,0 (topic 1) Flashcards

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1
Q

what is the name of the elements in group 0 of the periodic table

A

noble gases

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2
Q
A

the boiling points increase down the group

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3
Q

argon is in group 0, what type of particles are in a sample of argon

A

atoms

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4
Q
A
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5
Q

what is the name of the elements in group 7 of the periodic table

A

halogens

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6
Q
A
  • increase
  • increases
  • increase
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7
Q

hydrogen and chlorine react to produce hydrogen chloride, write down the balanced symbol equation for the reaction

A
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8
Q

suggest the conditions needed for hydrogen and iodine to react, explain the reason for your answer (2)

A
  • temperature greater than 200°C
  • iodine is less reactive than bromine
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9
Q

use your understanding of atomic structure to explain the trend in reactivity in the group 7 elements (3)

A
  • as you move down group 7, electrons in the outermost shell are further from the nucleus
  • forces are weaker
  • electrons are gained less easily
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10
Q

why does iodine have a higher boiling point than chlorine (1)

A

the forces between iodine molecules are stronger

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11
Q

astatine (At) is below iodine in Group 7, predict:
- the formula of an astatine molecule
- the state of astatine at room temperature (2)

A
  • At2
  • solid
  • astatine is a chemical element, and so does not have a molecular formula. It may occur as diatomic molecules, formula At2
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12
Q

sodium is a metal in group 1 of the periodic table, describe what you would see when sodium reacts with chlorine (2)

A
  • flame
  • white solid forms
  • (green) colour of chlorine gas disappears
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13
Q

the atomic number of potassium is 19, give the electronic structure of a potassium atom

A

2, 8, 8, 1

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14
Q

write down the balanced symbol equation for the reaction of potassium with water

A
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15
Q

state the trend in reactivity of the group 1 elements (1)

A

reactivity increases down the group

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16
Q

explain the trend in reactivity in terms of atomic structure of the group 1 elements

A
  • down group atoms get bigger
  • electrons further away from nucleus
  • outer electron more easily lost
17
Q
A
  • they react with oxygen
  • they have low melting points
18
Q

(6)

A

add chlorine to potassium bromide (max 2 marks):
- add aqueous chlorine to a solution of potassium bromide
- if the solution turns orange OR yellow
- bromine has been produced
- so chlorine is more reactive than bromine
add bromine to potassium iodide (max 2 marks):
- add aqueous bromine to a solution of potassium iodide
- if the solution turns yellow (or red or brown)
- iodine has been produced
- so bromine is more reactive than iodine
add chlorine to potassium iodide (max 2 marks):
- add aqueous chlorine to a solution of potassium iodide
- if the solution turns yellow OR red OR brown
- iodine has been produced
- so chlorine is more reactive than iodine

19
Q

explain how the reactivity of halogens changes going down group 7, use the results in the table above in your answer (3)

A
  • the reactivity decreases going down Group 7
  • because chlorine displaces bromine and iodine
  • and bromine displaces iodine
20
Q

write down the balanced symbol equation for the reaction of lithium and water, include state symbols

A
21
Q

explain why the group 1 metals are called the alkali metals (1)

A

group 1 metals react with water producing an alkaline solution

22
Q

state two observations that the student would make during the reaction of lithium reacting with water to produce lithium hydroxide and hydrogen (2)

A
  • bubbles/effervescence/fizzing
  • lithium disappears
  • lithium moves on the surface of the water
  • universal indicator turns purple
23
Q

explain why all group 1 metals have similar reactions with water (1)

A

all have one electron in their outer shell

24
Q

potassium is more reactive than lithium, explain why, in terms of electronic structure (3)

A
  • in potassium the outer shell electron is further away from the nucleus
  • therefore the outer shell electron is less strongly attracted to the nucleus
  • so the outer shell electron in potassium is more easily lost
25
Q

explain why group 1 metals are stored under oil (1)

A
  • oil acts as barrier between metal and air
  • because they are reactive
26
Q
A

chlorine is toxic

27
Q

the teacher weighed the glass tube and contents before the reaction and after the reaction, describe what happened to the mass of the glass tube and contents during the reaction,
explain your answer (2)

A
  • the mass increased
  • chlorine atoms are now part of solid iron chloride (the mass of the chlorine atoms is now also measured)
28
Q

predict what you would observe when fluorine gas reacts with iron (1)

A

burns very vigorously

29
Q

explain, in terms of electronic structure, why the reactivity of the halogens decreases going down group 7 (4)

A
  • group 7 elements gain one electron to achieve a full outer shell
  • going down group 7, there are more shells between the nucleus and the outer electron
  • so the force of attraction between the nucleus and outer electron decreases
  • and it becomes harder to gain the outer electron
30
Q

an atom of sodium has a mass number of 23, give the number of protons, neutrons and electrons in this atom of sodium

A
  • protons: 11
  • neutrons: 12
  • electrons: 11
31
Q

(6)

A

physical properties (max 3 marks):
- transition elements have high melting points
- group 1 elements have low melting points
- transition elements have high densities
- group 1 elements have low densities
- transition elements are hard
- transition elements are strong
- group 1 elements are soft
chemical properties (max 3 marks):
- transition elements have low reactivity
- group 1 elements are very reactive
- transition elements are used as catalysts
- group 1 elements are not used as catalysts
- transition elements form ions of different charges
- group 1 elements only form +1 ions
- transition elements form coloured compounds
- group 1 elements form white / colourless compounds

32
Q
A
  • bubbles (very) quickly
  • melts into a ball
  • floats
  • moves very quickly
  • flame
33
Q

the scientist concluded that, for group 1 elements, reactivity increases down the group, give two ways in which the scientist’s observations support her conclusion (2)

A
  • increasing speed of movement
  • increasing rate of bubble production
  • doesn’t melt ➔ melts
  • no flame ➔ flame (or flame ➔ explosion)
34
Q

write and balance the equation for the reaction of rubidium with water

A
35
Q
A

the noble gases have boiling points that increase going down the group

36
Q

explain why noble gases are monatomic (2)

A
  • outermost shell full
  • no tendency to lose or gain electrons
37
Q

give the word equation for the reaction of sodium with oxygen

A

sodium + oxygen ➔ sodium oxide

chemistry (paper one) (24 decks)

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