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*Gsce Science > Chemistry C1 And C2 > Flashcards

Chemistry C1 And C2 Flashcards

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1
Q

What was the early idea of an atom before electrons were discovered?

A

Atoms were thought to be tiny, indivisible spheres.

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2
Q

What are the relative masses of : protons neutrons and electrons

A

Proton:1
Neutron:1
Elctron:1/2000

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3
Q

What did the plum pudding model suggest about the atom?

A

The atom is a ball of positive charge with negative electrons embedded in it.

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4
Q

What experiment led to the rejection of the plum pudding model?

A

The alpha particle scattering experiment.

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5
Q

What did the alpha particle scattering experiment show?

A

The mass of an atom is concentrated in a tiny, positively charged nucleus.

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6
Q

What model replaced the plum pudding model?

A

The nucleus model of an atom

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7
Q

How do you find out the period and group of an element

A

Group:number of electrons in the outer shell
Period:total number of shells

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8
Q

What did later experiments reveal about the nucleus’s positive charge?

A

It is made up of smaller particles called protons.

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9
Q

Who provided evidence for the existence of neutrons?

A

james chadwick

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10
Q

How long after the nucleus was accepted did Chadwick discover neutrons?

A

About 20 years.

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11
Q

Why did the alpha particle scattering experiment lead to a change in the atomic model?

A

It showed that the atom has a dense, positively charged nucleus, not a diffuse ball of charge.

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12
Q

What is the relative charge of protons neutrons and electrons

A

Proton:1
Neutron:0
Electron:-1

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13
Q

How are elements arranged in the periodic table?

A

By increasing atomic (proton) number

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14
Q

How are compounds formed?

A

They are formed through chemical reactions which always involve the formation of one or more new substances

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15
Q

What are columns in the periodic table called

A

Groups.

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16
Q

Why is it called the periodic table?

A

Similar properties occur at regular intervals.

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17
Q

What do elements in the same group have in common?

A

The same number of outer electrons, giving them similar chemical properties.

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18
Q

What does an element’s position in the periodic table tell us about its electrons?

A

It shows the number of electron shells and outer electrons.

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19
Q

What does an element’s group tell us about its reactivity?

A

Elements in the same group have similar reactivity.

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20
Q

Where are the most reactive metals and non-metals found?

A

Metals bottom left
Non metals top right

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21
Q

How were elements first arranged in early periodic tables?

A

By atomic weights

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22
Q

What were the problems with early periodic tables?

A

They were incomplete, and some elements were placed in the wrong groups.

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23
Q

How did Mendeleev improve the periodic table?

A

He left gaps for undiscovered elements and reordered some elements based on properties.

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24
Q

What discovery explained issues with atomic weights?

A

The discovery of isotopes.

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25
Q

How do non-metals form ions?

A

Non-metals do not form positive ions.

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26
Q

How do metals form ions?

A

Metals form positive ions.

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27
Q

What are two physical properties of metals?

A

Good conductors of heat and electricity, malleable.

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28
Q

What are two physical properties of non-metals?

A

Poor conductors and brittle in solid form.

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29
Q

What are the names of group 1,7 and 0

A

Group 1: alkali metals
Group 7: halogens
Group 0: noble gases

30
Q

What is an atom?

A

Smallest part of an element that can exist

31
Q

What is a molecule?

A

Two or more non metal atoms that are bonded together

32
Q

What is an element?

A

A substance made up of a particular type of atom

33
Q

What is a compound?

A

Compounds are two or more elements that are chemically combined in fixed proportions

34
Q

What is the basic structure of an atom?

A

Atoms consist of a nucleus containing protons and neutrons, surrounded by electrons in shells.

35
Q

: How are elements ordered in the periodic table?

A

: How are elements ordered in the periodic table?

36
Q

What is a group in the periodic table?

A

A vertical column of elements with similar properties.

37
Q

What is a period in the periodic table?

A

A horizontal row of elements with increasing atomic numbers.

38
Q

How is electronic structure linked to the periodic table?

A

Elements in the same group have the same number of outer-shell electrons.

39
Q

What is an ion?

A

An ion is an atom or group of atoms that has an electric charge.

40
Q

Why do the first three Group 1 metals float on water?

A

They are less dense than water.

41
Q

What happens when Group 1 metals react with water?

A

They produce hydrogen gas and a metal hydroxide.

42
Q

Why are Group 1 metals stored in oil?

A

To prevent reactions with air or water.

43
Q

What ions do Group 1 metals form?

A

+1 ions.

44
Q

Name the first four elements in Group 7.

A

Fluorine, chlorine, bromine, iodine.

45
Q

Why do Group 7 elements react similarly?

A

They all have seven electrons in their outer shell.

46
Q

What is an isotope

A

Isotopes are atoms of the same element with the same number of protons but different number of neutrons in the nucleus.

47
Q

Why are noble gases unreactive?

A

They have full outer electron shells.

48
Q

What is the trend in noble gas boiling points?

A

Boiling points increase down the group.

49
Q

How can trends in the periodic table be predicted?

A

By examining group and period positions.

50
Q

What stable ions do the first 20 elements form?

A

They form ions to achieve a full outer shell.

51
Q

: How is the electronic structure of metals different from non-metals?

A

Metals lose electrons; non-metals gain electrons.

52
Q

How does electronic structure affect reactivity?

A

Metals lose electrons easily; non-metals gain them easily.

53
Q

Why do Group 7 elements react similarly?

A

They all have seven electrons in their outer shell

54
Q

What ions do Group 7 non-metals form when reacting with metals?

A

-1 ions.

55
Q

What is the trend in reactivity in Group 7?

A

Reactivity decreases down the group.

56
Q

What are the main properties of halogens?

A

They are colored, diatomic, and become less reactive down the group.

57
Q

What happens in a halogen displacement reaction?

A

A more reactive halogen displaces a less reactive halogen from a compound.

58
Q

How do you compare reactivity in Group 7?

A

By observing how quickly halogens react with other substances.

59
Q

What is the trend in reactivity in Group 1?

A

Reactivity increases down the group.

60
Q

How does electronic structure affect reactivity in Group 1?

A

Outer electrons are farther from the nucleus, so they are lost more easily.

61
Q

Why are Group 1 and Group 7 elements reactive?

A

Group 1 loses electrons easily; Group 7 gains electrons easily.

62
Q

Why are Group 1 and Group 7 elements reactive?

A

Group 1 loses electrons easily; Group 7 gains electrons easily.

63
Q

How does the nuclear model explain reactivity trends?

A

Outer electrons feel less attraction to the nucleus as the atom gets larger.

64
Q

What is the trend in reactivity for Group 2?

A

Reactivity increases down the group.

65
Q

What is the trend in reactivity for Group 6?

A

Reactivity decreases down the group.

66
Q

What are the typical properties of transition metals?

A

They are strong, dense, good conductors, and form colorful compounds.

67
Q

How do Group 1 metals compare with transition metals?

A

Group 1 metals are softer, less dense, and more reactive.

68
Q

Why is mercury not a typical transition metal?

A

It is liquid at room temperature and has less variable oxidation states.

69
Q

Why might a transition metal or compound be used?

A

For its strength, conductivity, or as a catalyst.

70
Q
A

*Gsce Science (3 decks)

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