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GCSE Chemistry > C1 > Flashcards

C1 Flashcards

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1
Q

Summarize the Daltons Model of the Atom

A

Atoms are tiny spheres that cannot be broken down.

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2
Q

Summarize the Plum Pudding Model

A

The atom is a ball of spread out positive charge with negative electrons embedded into it

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3
Q

Summarize the Nuclear Model

A

The atom is a ball of spread out positive charge with negative electrons embedded into it

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4
Q

Summarize the Electron Shell Model (Bohr Model)

A

Electrons orbit the nucleus at a fixed energy level

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5
Q

What are the beliefs of Protons and Neutrons

A

The nucleus consists of protons which have a positive charge and neutrons which have no charge

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6
Q

What is the radius of an atom

A

1x 10-10m

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7
Q

What is the radius of an Nucleus

A

1 x 10-14 m

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8
Q

If a substance is made up of one type of atom what is it called?

A

An element

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9
Q

What does Atomic Number tell us

A

Amount of Protons in an atom

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10
Q

What does Mass number tell us

A

Number of Protons and neutrons

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11
Q

How do we work out the number of neutrons in an atom

A

mass number - atomic number

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12
Q

What is an isotope

A

Two of the same atoms with same number of protons but different number of neutrons

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13
Q

how do we work out relative atomic mass of an isotope

A

(Abundance of isotope 1 x Mass of isotope 1) + (Abundance of isotope 2 x Mass of isotope 2)
÷100

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14
Q

In terms of electrons, what is the difference between the plum pudding and the nuclear model?

A

Electrons in the Plum Pudding Model are ‘embedded inside the atom’. Nuclear model, the Electrons are orbiting on outer shells

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15
Q

What are 2 different atoms chemically bonded together called?

A

A compound

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16
Q

Name Separation techniques

A

Paper Chromatography, Filtration, Crystallisation, Distillation, Fractional Distillation

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17
Q

What does Paper chromatography separate

A 
Soluble substances from a mixture using a suitable solvent 
For example (Dyes in an ink)
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18
Q

What does Filtration separate

A 
Insoluble solids from a liquid 
For Example (Sand from Water)
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19
Q

What does crystallization separate

A 
Soluble substances from a solution 
For example (Salt from Saltwater)
20
Q

What does distillation separate

A 
Liquids from solutions
For Example (Water from Saltwater)
21
Q

What does Fractional Distillation separate

A 
A mixture of liquids due to the liquids having different boiling points.  
For Example (Ethanol from a mixture of ethanol and water, Fractions in Crude oil)
22
Q

What does it mean if the symbols are in brackets

A

If symbols are in brackets, then you must multiply everything in the brackets by the little number that follows them. For example:
Mg(OH)2 has one magnesium atom. The O and H are in brackets so must be multiplied by 2.

23
Q

What is Conservation of Mass

A

In any chemical reaction, the atoms are neither created nor destroyed. It does not matter whether the reaction is hot or cold, the atoms cannot be created or destroyed. But they are rearranged.

24
Q

How is the Table of Elements arranged

A

By Atomic Number

25
Q

Why do elements in the same group have similar properties

A

Because they have the same number of electrons in their outer shells

26
Q

Metals all ____ their outer shell electrons to form a positive ion

A

Lose

27
Q

Non-Metals will ____ electrons to form a stable outer shell when reacting with metals to form a negative ion

A

Gain

28
Q

Positive and negative ions will be electrostatically attracted and form an _____ bond between the ions.

A

Ionic

29
Q

Group 1 metals are known as what

A

Alkali Metals

30
Q

Alkali Metals react with

A

Oxygen to form oxides
Chlorine to form chlorides
Water to form hydroxides

31
Q

In which direction do group 1 metals increase in reactivity

A

They increase in reactivity going down the group

32
Q

In order to react, the metal needs to lose an electron. The easier it is to lose, the more ________ it will be

A

Reactive

33
Q

Group 7 elements are also known as the

A

Halogens

34
Q

What are Halogens

A

They are reactive non-metals that form as diatomic (two atoms joined together by sharing electrons (we call this a COVALENT bond).

35
Q

In which direction does the reactivity of Group 7 elements increase and why

A

The reactivity of the halogens increases up the group
In order to react, the halogen needs to gain an electron. The easier it is to gain, the more reactive it will be.
Closer the outer shell to the nucleus, easier for the atom to gain an electron

36
Q

What are Group 0 Elements known as

A

The Noble gases
They have full outer shells which means they do not need to gain or lose electrons. They all have 8 electrons in the outer shell, EXCEPT FOR HELIUM WHICH ONLY HAS 2.

37
Q

Why do the Noble gases not react with other elements

A

They have full outer shell and unlike other gases, they exist naturally as single atoms

38
Q

In which direction does the boiling point of Noble Gases increase

A

Going down the group

39
Q

What are the transition metals

A

The metals in between group 2 and group 3
They share similar physical properties with other metals, such as: they conduct electricity in both liquid and solid state and they are often shiny.

40
Q

How do the Alkali metals react with Oxygen

A

React quickly with Oxygen in the air at room temperature.

41
Q

How do the Alkali metals react with Water

A

React vigorously with cold water.

42
Q

How do the Alkali Metals react with the Halogens

A

React vigorously with the halogens.

43
Q

How do the Transition Metals react with Oxygen

A

Most react slowly or not at all. Some transition metals such as Copper or Iron react with Oxygen on heating.

44
Q

How do the Transition Metals react with Water

A

Iron reacts slowly with water and Oxygen to form hydrated Iron (III) oxide, or rust.

45
Q

How do the Transition Metals react with The Halogens

A

Some transition metals, such as Iron react with halogens.

46
Q

What are some Transition Metals used for

A

Used in catalysts to speed up chemical reactions without being used up. Eg/ Manganese (VI) Oxide increases the decomposition of hydrogen peroxide to oxygen and water.

47
Q

Do the metals in group 1 of the periodic table have a high or a low density?

A

Low

GCSE Chemistry (16 decks)

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