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Chemistry from book questions > Topic 1-5 > Flashcards

Topic 1-5 Flashcards

1
Q

Sketch an atom, Label the nucleus and the electrons.

A

Phone//

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2
Q

What is the charge of a proton?

A

+1

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3
Q

True or false? Elements contain more than one type of atom.

A

False

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4
Q

Give the formula for:

a)Carbon dioxide b)Sodium carbonate

A

C02

Na2CO3

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5
Q

Balance these equations:

a)Mg + O2 —> MgO b) H2SO4 +Na2SO4 +H2O

A

a) 2MgO

b) H2SO4 +2NaOH —> Na2SO4 +2H20

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6
Q

What is the difference between a compound and a mixture?

A

Mixtures are easily separated unlike compounds.

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7
Q

What is the name of the pattern formed from carrying out paper chromatography?

A

Pattern of spots called chromatogram

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8
Q

Which method of separation is useful to separate an insoluble solid from a liquid.

A

Filtration

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9
Q

Which method of distillation would you use to separate a soluble solid from a liquid.

A

Evaporation

Crystallisation

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10
Q

Which method of distillation would you use to separate liquids with similar boiling points?

A

Fractional distillation

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11
Q

Who discovered that the plum pudding model was wrong?

A

Rutherford

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12
Q

Who first devised an experiment that proved the existence of the neutron?

A

James Chadwick, evidence for neutral particles in the nucleus.

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13
Q

What is the electronic structure of sodium?

A

2,8,1

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14
Q

Why did Mendeleev leave gaps in his Table of Elements?

A

For undiscovered elements.

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15
Q

How are the group number and the number of electrons in the outer shell of an element related?

A

The group number is the number of electrons in outer shell.

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16
Q

What kind of ions do metals form?

A

Ionic bond

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17
Q

Where are non-metals on the periodic table?

A

Right side

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18
Q

Give three properties which are specific to transition metals.

A

More than one ion
Often coloured
Make good catalysts.

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19
Q

State three trends as you go down Group 1.

A

Increasing reactivity
Lower melting + boiling points
Higher relative atomic mass

20
Q

State the products of the reaction of sodium and water.

A

sodium hydroxide + hydrogen

21
Q

State the differences between Group 1 and transition metals for the following properties:

a) Hardness
b) Reactivity
c) Melting Points

A

a) group 1 less hard
b) group 1 more reactive
c) group 1 lower melting points

22
Q

How do the boiling points of halogens change as you go down the group from fluorine to astatine?

A

Higher melting and boiling points

23
Q

What is the change of the ions that halogens form when they react with metals?

A

1- ions called halides, ionic structure

24
Q

Predict whether iodine is displaced by chlorine in a solution of potassium iodide.

A

Yes, iodine is displaced by chlorine.

25
Q

What is the trend in boiling point as you go down group 0?

A

Boiling point increases as you go down.

26
Q

What type of ion do elements from each of the following groups form?

a) Group 1
b) Group 2

A

a)group 1 and 2 loses electrons and forms a positive ion.

27
Q

Describe how an ionic bond forms.

A

When a metal and non metal react together, the metal atom loses electrons to form a positively charged ion and the non-meal gains these electrons to form a negatively charged ion.

28
Q

Sketch dot and cross diagrams to show the formation of:

a) hydrogen
b) water
c) hydrogen chloride

A

PHONE//

29
Q

List the main properties of ionic compounds.

A

High melting points and high boiling points
When they melt they can carry electric current
Dissolve easily in water

30
Q

Describe how covalent bonds form.

A

Non metal atoms bond together to share pairs of electrons to make covalent bonds

31
Q

Sketch dot and cross diagrams showing the bonding in a molecule of:

a) hydrogen
b) water
c) hydrogen chloride

A

PHONE

32
Q

Explain why simple molecular compound typically have low melting and boiling points.

A

Only need to break feeble intermolecular forces and not the covalent bonds.

33
Q

Describe the structure of a polymer.

A

Polymers are Long chains of repeating units.

34
Q

Give three examples of giant covalent substances.

A

Diamond
Graphite
Silicon dioxide

35
Q

Explain why graphite can conduct electricity.

A

Has a delocalised electron

36
Q

Explain how fullerenes could be used to deliver drugs into the body.

A

Can be used to cage other molecules.

37
Q

What is metallic bonding?

A

Involves delocalised electrons.

There are strong forces of electrostatic attraction between the positive metal ions and the shared negative electrons.

38
Q

List three properties of metals and explain how metallic structure causes each property.

A

Solid at room temperature
Good Conductors of electricity and heat
Malleable

39
Q

Explain why alloys are harder than pure metals.

A

When another element is mixed with a pure metal, the new metal atoms will distort the layers of metal atoms, making it more difficult form them to slide over each other.

40
Q

Name the three states of matter.

A

Solid
Liquid
Gas

41
Q

What is the state symbol of an aqueous substance?

A

(aq)

42
Q

What is the name of the temperature at which a liquid becomes a gas?

A

Boiling point

43
Q

How does the strength of the forces between particles influence the temperature at which a substance changes state?

A

The stronger the forces, the more energy is needed to break them, and so the higher the meting and boiling points of the substance.

44
Q

What is nano science?

A

The investigation of the uses and properties of nanoparticles, called nanoscience.

45
Q

Give three uses of nanoparticles.

A

Make new catalysts
Nanomedicine
Deodrants

46
Q

Explain why people may be wary of using products that contain nanoparticles.

A

Effects of nanoparticles on Health Aren’t fully understood.

Chemistry from book questions (1 decks)

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