1.1 Atomic structure Flashcards

1
Q

Who are the three scientists that developed an atomic model in order.

A

.John Dalton
.J.J Thomson
.Ernest Rutherford

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2
Q

What was Daltons three part Atomic theory?

A

.All substance are made of atoms-Atoms cannot be created, divided or destroyed.
.Atoms of the same element are alike and atoms of different elements are different
.Atoms join together to make new substances

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3
Q

What discovery caused the original Dalton model of an atom to change?

A

The subatomic particle

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4
Q

How did JJ Thomson discover the electron?

A

He experimented with a cathode ray tube

The beam moved towards the positively charged plate so he knew that particles must have a negative charge

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5
Q

Describe the atomic model proposed by JJ Thomson

A

.Plum Pudding model

Negatively charge electrons scattered through a positively charged material

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6
Q

What did Ernest Rutherford discover from his gold foil experiment?

A

.Most of the particles shot straight through suggesting that an atom is mostly empty space
.A few particles were deflected and a few bounced back showing there must be a tiny dense positively charged Nucleus

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7
Q

Describe Rutherford’s new model of the atom

A

.Mass is concentrated in the central nucleus
.Mostly empty space
.Electrons travel in random paths around the nucleus

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8
Q

Describe the structure of an atom

A

.Small central nucleus made up of protons and neutrons

.Electrons orbit the nucleus in cells

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9
Q

What are the relative masses of the subatomic particles?

A

Proton-+1
Neutron-0
Electron- -1

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10
Q

What are the relative masses of the three subatomic particles?

A

Proton= 1
Neutron-1
Electron= 1/1836

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11
Q

Why do atoms contain an equal number of protons and electrons?

A

The charges cancel out as atoms are neutral

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12
Q

Compared to the rest of the atom, how large is the nucleus?

A

It is very small

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13
Q

Where is most of the mass concentrated in an atom?

A

The Nucleus

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14
Q

Give the equation to work out the mass number

A

Number of Protons+Neutrons

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15
Q

What are Isotopes?

A

.These are different atoms of the same element containing the same number of protons but different numbers of neutrons in their nuclei

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16
Q

What does the Atomic number allow you to calculate?

A

Number of protons

17
Q

How would you calculate the number of neutrons

A

Mass number-Atomic number

18
Q

How does the existence of Isotopes results in the relative atomic mass of some elements not being whole numbers?

A

.Different number of neutrons
.RAM is calculated using an abundance of isotopes and because it is an average it can lead to it not being a whole number

19
Q

How do you calculate the R.A.M of an element from their relative masses and isotopes?

A

(mass of isotope-A x % of isotope-A) + (mass of isotope-B x % of isotope-B)
100