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Chemistry > Atomic structure *DOUBLE AND TRIPLE* > Flashcards

Atomic structure *DOUBLE AND TRIPLE* Flashcards

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1
Q

What A is all matter made of?

A

atoms

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2
Q

Which scientist first came up with a model of what atoms are like?

A

Dalton

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3
Q

How did Dalton describe atoms?

A

tiny indestructible spheres

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4
Q

How did Dalton use his model to explain elements?

A

all the atoms in an element were identical (and different to atoms of other elements)

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5
Q

How have Dalton’s ideas about atoms changed?

A

atoms are not indestructible but are made up of smaller particles (however atoms are the smallest part of an element that can exist)

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6
Q

The discovery of the electron by Thomson led to which model of the atom?

A

plum pudding model

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7
Q

Describe the plum pudding model.

A

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

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8
Q

Describe the alpha particle scattering experiment.

A

positively charged alpha particles were scattered by gold foil - some passed straight through, some where deflected and some were repelled back

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9
Q

What was concluded from the alpha particle scattering experiment?

A

the mass of an atom was concentrated at the centre of the atom and the centre (nucleus) was positively charged - this is known as the nuclear model of the atom

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10
Q

How did Niehls Bohr adapt the nuclear model?

A

suggested that electrons orbit the nucleus at specific distances in fixed energy levels or shells

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11
Q

Who provided evidence showing the existence of neutrons?

A

James Chadwick

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12
Q

What is the difference between an atom and a molecule?

A

molecules contain two or more atoms chemically joined together in a group

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13
Q

What are the names of the three main subatomic particles?

A

protons, neutrons, electrons

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14
Q

What tiny particles flow in an electric current?

A

electrons

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15
Q

What charge do electrons particles have?

A

negative

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16
Q

What is the nucleus of an atom?

A

tiny central part of an atom made up of protons and neutrons

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17
Q

How are electrons arranged in an atom?

A

circling/orbiting the nucleus in regions called shells

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18
Q

How do protons and electrons compare in terms of relative charge?

A

protons have a positive (+1) charge and electrons have a negative (-1) charge

19
Q

Why are atoms neutral?

A

they have the same number of protons and electrons and so equal positive and negative charges

20
Q

What is the relative charge of a neutron?

A

neutral

21
Q

What is the fundamental difference between atoms of different elements?

A

they contain different numbers of protons

22
Q

How does the size of a nucleus compare to the size of the atom?

A

the nucleus is tiny compared to the size of the atom, 1/10 000 the size of an atom, or about 1x10-14m

23
Q

What is the radius of an atom?

A

0.1nm or 1x10-10m

24
Q

What is the relative mass of a proton?

A

1

25
Q

What is the relative mass of a neutron?

A

1

26
Q

What is the relative mass of an electron?

A

0 or very small

27
Q

How many protons are there in an atom with an atomic number of 26?

A

26

28
Q

How many neutrons are there in an atom with an atomic number of 26 and a mass number of 56?

A

30

29
Q

What does the atomic number of an atom tell you about its structure?

A

the number of protons in an atom

30
Q

What does the mass number of an atom equal?

A

the number of protons plus the number of neutrons

31
Q

What will be the same about atoms of the same element?

A

they will have the same atomic number and same number of protons

32
Q

Where is most of the mass of an atom found?

A

in the nucleus

33
Q

How many electrons are in an atom with a mass number of 65 and an atomic number of 30

A

30

34
Q

How many protons, neutrons and electrons are in an atom that has an atomic number of 13 and a mass number of 27?

A

13 protons, 14 neutrons, 13 electrons

35
Q

What are isotopes?

A

Atoms with the same number of protons but a different number of neutrons. This means atoms will share the same atomic number but have a different atomic mass.

36
Q

What type of atom is used as the standard for comparing masses and working out relative atomic masses of elements?

A

carbon-12

37
Q

What is the relative atomic mass of an element?

A

average mass value for the element that takes account of the abundance of isotopes of the element

38
Q

Where are electrons found in an atom?

A

around the nucleus/in shells/in energy levels

39
Q

Where are the shells found in an atom?

A

around the nucleus

40
Q

How many electrons can occupy the first four electron shells, to a maximum of 20 electrons?

A

2,8,8,2

41
Q

What is the electronic structure of sodium? (atomic number = 11)

A

2,8, 1

42
Q

What is the electronic structure of chlorine? (atomic number = 17)

A

2, 8,7

43
Q

The atomic number of oxygen is 16. How many electrons do its atoms have?

A

16

44
Q

What is the electronic structure of magnesium? (atomic number = 12)

A

2,8,2

Chemistry (7 decks)

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