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GCSE Science AQA 2016 Onwards > Fundamental Chemistry > Flashcards

Fundamental Chemistry Flashcards

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1
Q

Define compound

A

Two or more elements chemically bonded

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2
Q

Define element

A

Substance made up of only one type of atom

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3
Q

Mass of a proton

A

1 AMU

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4
Q

Mass of a neutron

A

1 AMU

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5
Q

Mass of an electron

A

Almost 0, 1/2000 AMU

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6
Q

Define mass number

A

Number of protons + neutrons

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7
Q

Define atomic number

A

Number of protons (in the nucleus)

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8
Q

Explain how a chlorine atom becomes a chlorine ion

A

Gains one electron

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9
Q

Explain how a sodium atom becomes a sodium ion

A

Loses one electron

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10
Q

Explain how an oxygen atom becomes an oxide ion

A

Gains two electrons

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11
Q

Explain how a magnesium atom becomes a magnesium ion

A

Loses two electrons

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12
Q

Charge of a proton

A

+1

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13
Q

Charge of a neutron

A

0

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14
Q

Charge of an electron

A

-1

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15
Q

Define a molecule

A

Two or more atoms bonded together

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16
Q

Formula of sodium hydroxide

A

NaOH

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17
Q

Formula of magnesium chloride

A

MgCl2

18
Q

John Newlands and Mendeleev arranged their periodic table in order of…

A

atomic mass

19
Q

The modern periodic table is arranged in order of…

A

atomic number (proton number)

20
Q

Explain why Mendeleev left gaps in his periodic table

A

to make the pattern fit for undiscovered elements

21
Q

Explain why potassium and sodium are in the same group of the periodic table

A

They both have one electron in their outer shell They react similarly

22
Q

Describe how alkali metals react with water

A

-Bubble/Fizz/Effervesce -Turn indicator purple -Move about on the surface of the water -Sodium melts in a ball -Potassium burns with a lilac flame

23
Q

Write a symbol equation for the reaction of sodium with water

A

2Na + 2H2O –> 2NaOH + H2

24
Q

Name the typical properties of transition metals

A

-Good conductors of heat and electricity -Hard and strong -High density -High melting point -Form coloured compounds -Form ions with different charges (i.e. Fe2+ and Fe3+

25
Q

Name one similarity and difference between the properties of copper and lithium

A

Similarities - conduct electricity Differences - lithium is more reactive, lithium is less dense, lithium is softer, lithium has a lower melting point

26
Q

Describe the trend in reactivity of the group 1 metals as you go down the group

A

Reactivity increases

27
Q

Describe the trend in melting point as you go down group 7

A

Melting point increases (fluorine is a gas, iodine is a solid)

28
Q

Describe the trend in reactivity as you go down group 7

A

Reactivity decreases

29
Q

Explain why chlorine and bromine are group 7 of the periodic table

A

Both have 7 electrons in their outer shell

30
Q

Finish the following word equation Bromine + potassium iodide –>

A

Potassium bromide + iodine

31
Q

Explain why chlorine can displace bromine from potassium bromide

A

chlorine is more reactive

32
Q

Name the ion that turns universal indicator purple

A

OH-

33
Q

Explain why potassium is more reactive than sodium

A

-Potassium has a greater atomic radius/more energy levels/more shells -there is less attraction between the outer electron and the nucleus/more shielding -Potassium loses an electron easier

34
Q

Explain why fluorine is more reactive than chlorine

A

-Fluorine has a smaller atomic radius/less energy levels/less shells -there is greater attraction between the outer shell and the nucleus/less shielding -fluorine gains an electron easier

35
Q

Name one use for the transition metals

A

Catalysts

36
Q

Name pieces of apparatus A, B, C

What is the name of this separation process?

A

A = thermometer

B = condenser

C = (round bottomed) flask

Fractional Distillation

37
Q

A student is given a mixture of salt and sand. Describe a method the student could do to separate the mixture naming the apparatus they should use.

A
  • Pour the mixture into a beaker
  • Add water to the beaker
  • Stir until the salt dissolves
  • Filter the mixture
  • Remove the residue (sand)
  • Dry the sand in an oven
  • Place the filtrate (salt solution) in an evaporating basin
  • Heat the solution with a Bunsen burner until the water evaporates
  • Cool and dry the salt with an oven
38
Q

Explain why chlorine’s relative atomic mass is 35.5

A

Relative atomic mass is an average mass

Chlorine exists as Cl- 35 and Cl-37

75% is Cl-35 and 25% is Cl-37

(35 x 75 ÷ 100) + (37 x 25 ÷ 100) = 35.5

39
Q

Explain why Mendeleev swapped Tellurium and Iodine’s position in his periodic table.

A
  • Iodine has similar properties to other group 7 elements
  • Iodine had similar chemical reactions to other group 7 elements
  • Iodine is also diatomic
40
Q

What subatomic particle did James Chadwick discover?

A

Neutron

41
Q

How did Mendeleev’s periodic table become accepted by scientists?

A

They discovered the elements he’d left gaps for

and they had similar properties to those he’d precited

GCSE Science AQA 2016 Onwards (12 decks)

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