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*Gsce Science > Chemistry C1 And C2 > Flashcards

Chemistry C1 And C2 Flashcards

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
How do non-metals form ions?
Non-metals do not form positive ions.
26
How do metals form ions?
Metals form positive ions.
27
What are two physical properties of metals?
Good conductors of heat and electricity, malleable.
28
What are two physical properties of non-metals?
Poor conductors and brittle in solid form.
29
What are the names of group 1,7 and 0
Group 1: alkali metals Group 7: halogens Group 0: noble gases
30
What is an atom?
Smallest part of an element that can exist
31
What is a molecule?
Two or more non metal atoms that are bonded together
32
What is an element?
A substance made up of a particular type of atom
33
What is a compound?
Compounds are two or more elements that are chemically combined in fixed proportions
34
What is the basic structure of an atom?
Atoms consist of a nucleus containing protons and neutrons, surrounded by electrons in shells.
35
: How are elements ordered in the periodic table?
: How are elements ordered in the periodic table?
36
What is a group in the periodic table?
A vertical column of elements with similar properties.
37
What is a period in the periodic table?
A horizontal row of elements with increasing atomic numbers.
38
How is electronic structure linked to the periodic table?
Elements in the same group have the same number of outer-shell electrons.
39
What is an ion?
An ion is an atom or group of atoms that has an electric charge.
40
Why do the first three Group 1 metals float on water?
They are less dense than water.
41
What happens when Group 1 metals react with water?
They produce hydrogen gas and a metal hydroxide.
42
Why are Group 1 metals stored in oil?
To prevent reactions with air or water.
43
What ions do Group 1 metals form?
+1 ions.
44
Name the first four elements in Group 7.
Fluorine, chlorine, bromine, iodine.
45
Why do Group 7 elements react similarly?
They all have seven electrons in their outer shell.
46
What is an isotope
Isotopes are atoms of the same element with the same number of protons but different number of neutrons in the nucleus.
47
Why are noble gases unreactive?
They have full outer electron shells.
48
What is the trend in noble gas boiling points?
Boiling points increase down the group.
49
How can trends in the periodic table be predicted?
By examining group and period positions.
50
What stable ions do the first 20 elements form?
They form ions to achieve a full outer shell.
51
: How is the electronic structure of metals different from non-metals?
Metals lose electrons; non-metals gain electrons.
52
How does electronic structure affect reactivity?
Metals lose electrons easily; non-metals gain them easily.
53
Why do Group 7 elements react similarly?
They all have seven electrons in their outer shell
54
What ions do Group 7 non-metals form when reacting with metals?
-1 ions.
55
What is the trend in reactivity in Group 7?
Reactivity decreases down the group.
56
What are the main properties of halogens?
They are colored, diatomic, and become less reactive down the group.
57
What happens in a halogen displacement reaction?
A more reactive halogen displaces a less reactive halogen from a compound.
58
How do you compare reactivity in Group 7?
By observing how quickly halogens react with other substances.
59
What is the trend in reactivity in Group 1?
Reactivity increases down the group.
60
How does electronic structure affect reactivity in Group 1?
Outer electrons are farther from the nucleus, so they are lost more easily.
61
Why are Group 1 and Group 7 elements reactive?
Group 1 loses electrons easily; Group 7 gains electrons easily.
62
Why are Group 1 and Group 7 elements reactive?
Group 1 loses electrons easily; Group 7 gains electrons easily.
63
How does the nuclear model explain reactivity trends?
Outer electrons feel less attraction to the nucleus as the atom gets larger.
64
What is the trend in reactivity for Group 2?
Reactivity increases down the group.
65
What is the trend in reactivity for Group 6?
Reactivity decreases down the group.
66
What are the typical properties of transition metals?
They are strong, dense, good conductors, and form colorful compounds.
67
How do Group 1 metals compare with transition metals?
Group 1 metals are softer, less dense, and more reactive.
68
Why is mercury not a typical transition metal?
It is liquid at room temperature and has less variable oxidation states.
69
Why might a transition metal or compound be used?
For its strength, conductivity, or as a catalyst.
70

*Gsce Science (3 decks)

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