Structure Of The Atom YEAR TEN Flashcards

1
Q

In Thompsons experiment how did he show the electrons had a negative charge?

A

The electron beam was attracted towards the positive plate therefore they must be negatively charged. The particles were approximately 2000 times lighter than hydrogen atom and he called them electrons

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2
Q

How did Thomson suggest that the atom was neutral

A

It contained equal numbers of positive and negative charges and these cancelled each other out

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3
Q

How does the mass of a neutron compare with the mass of a proton

A

Mass of neutron (1) is equal to the mass of a proton (1)

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4
Q

How is the atom composed

A

Atom is composed of small, dense, positively, charged nucleus at the centre composed of protons and neutrons (most of the mass) with negatively charged electrons in shells orbiting the nucleus

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5
Q

What’s the relative mass of a proton

A

1

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6
Q

Relative mass of a neutron

A

1

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7
Q

Relative mass of a electron

A

1/1840

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8
Q

Relative charge of. A proton and neutron

A

Proton =+1
Neutron= 0

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9
Q

Relative charge of a electron

A

-1

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10
Q

How big is the radius of a atom

A

0.1nm

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11
Q

How big is the radius of a nucleus of an atom compared to the radius of an atom

A

1/10,000 of the radius of a atom

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12
Q

What is the definition of the atomic number

A

This is the number of protons in (the nucleus of) an atom

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13
Q

What’s the definition of the mass number

A

This is the total number of protons and neutrons in (the nucleus of) an atom

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14
Q

How do the atoms of one element differ from those of another

A

The number of protons electrons + neutrons found in each atom are different

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15
Q

What’s the definition of a element

A

Element is a substance that consists of only one type of atom and it cannot be broken down into anything simpler by chemical means

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16
Q

The number of protons in a atom is equal to its

A

Atomic number

17
Q

As an atom is electrically neutral (no overall charge) then the number of

A

Electrons must equal the number of protons

18
Q

The number of neutrons in an atom is equal to its

A

Mass no- atomic number

19
Q

Atoms with electric charges are called

A

Ions

20
Q

Atoms with positive charges are called

A

Cation

21
Q

Atoms with a negative charged are called

A

Anions

22
Q

What’s the formation of a cation

A

It’s the loss of electrons ( the symbol is +)

23
Q

What’s the formation of anions

A

It’s gaining electrons (symbol is -)

24
Q

What are isotopes

A

Isotopes are atoms which has The same number of protons (so they are atoms of the same element) but they have different number of neutrons (so they have a different mass number)

25
Q

How do you calculate isotopes

A

(It’s the percentage times the top number + the same again ) that equation divided by 100 gives you the answer

26
Q

How do you identify isotopes

A

It needs the same protons and electrons and different neutrons

27
Q

What’s not found in the nucleus of an atom

A

The electrons

28
Q

How is the periodic table arranged

A

By atomic number

29
Q

If an element has an atomic number of 12 how many protons and electrons does it have

A

12

30
Q

What did jj Thompson propose

A

The plum pudding model which stated that the negative electrons were embedded in a positive sphere (like the raisins in a plum pudding)

31
Q

What did Aristotle propose

A

He believed that matter was composed by four elements air fire earth and water