Atomic Structure Flashcards

(33 cards)

1
Q

Atomic structure History: Democritus

A

-around 500BC
-made atomic theory

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2
Q

What was the atomic theory?

A

-idea that everything is made up of tiny particles that can’t be broken down any further (atoms)
>particles separated by empty space

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3
Q

Atomic Structure History: John Dalton

A

-1803
-was the first to challenge Democritus’ atomic theory

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4
Q

What did John Dalton say about atoms?

A

-described atoms as solid sphere
-different types of spheres would make up different elements

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5
Q

Atomic Structure History: JJ Thompson

A

-1897
-came up with the plum pudding model

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6
Q

What change did JJ Thompson make to John Dalton’s theory?

A

-he said that the atoms couldn’t simply be solid spheres
-that they contained negatively charged particles (we now know as electrons)

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7
Q

What was the plum pudding model?

A

-theory that atoms are a ball of positive charge with electrons embedded in it

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8
Q

Atomic Structure History: Ernest Rutherford

A

-1909
-came up with nuclear model after conducting gold foil experiment

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9
Q

What was the nuclear model?

A

-theory that the atom had some sort of compact nucleus (that contained all of the positive charge)
-negative charge existed as some sort of cloud around the nucleus

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10
Q

What was the gold foil experiment?

A

> beam of +charged alpha particles passed through gold foil
-most went straight through the foil as expected (detected by a fluorescent screen)
ones shot towards the centre of gold foil went in unexpected angles, some even shot back in the same direction which they came from, meaning there was a compact centre of positive charge (nucleus)
-around nucleus, was mainly empty space with some electrons orbiting around it

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11
Q

Atomic Structure History: Niels Bohr

A

-1913
-fixed flaws to the rutherford model

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12
Q

What was Niels Bohr’s theory?

A

-that electrons orbited the nucleus in shells
-it was important as the orbiting of electrons stops them from being attracted to + nucleus and collapsing

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13
Q

Atomic Structure History: James Chadwick

A

-1932
-provided evidence that there are neutral particles in a nucleus (neutrons) after ernest rutherford discovered the protons

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14
Q

Neutron

A

-subatomic particle with neutral charge (0)
-relative mass is one

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15
Q

Proton

A

-subatomic particle with positive charge
(+1)
-relative mass is one

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16
Q

Electron

A

-subatomic particle with negative charge (-1)
-very small mass

17
Q

Nucleus and shells of atom

A

-atom has central nucleus
>nucleus is surrounded by electrons orbiting it in shells

18
Q

Atomic number

A

-found at the bottom of element on periodic table
-show the number of protons (or electrons) in an atom

19
Q

All atoms of a given element have the same number of…
Atoms of different elements have…

A

….protons.
…different numbers of protons.

20
Q

An atom contains equal numbers of protons and electrons. True or False

21
Q

What is an atom’s mass number?

A

-number of protons and neutrons found in the nucleus of an atom
-found at the top of the element

22
Q

How do we find out the number of protons in an atom?

A

-look at its atomic number

23
Q

How do we find out the number of electrons in an atom?

A

-look at its atomic number

24
Q

How do we find put the number of neutrons in an atom?

A

-do
mass number - atomic number (number of protons)

25
The atomic number of a sodium atom is 11 and its mass number is 23. Calculate the number of protons, neutrons and electrons it contains
-protons = 11 -electrons = 11 -neutrons = 23- 11 =12
26
What is an isotope?
-atoms of an element with same number of protons but different number of neutrons
27
What is it called when atoms of the same element have the same number of protons but different numbers of neutrons?
-Isotopes
28
One thing that is the same about an isotope compared to its atom and one thing that is different
-same > atomic number -different > mass number
29
Isotopes are harder or softer?
-harder
30
What is relative atomic mass?
-mean relative mass of the atoms of the different isotopes in element
31
What is relative atomic mass compared to?
-carbon-12 atom
32
How to calculate relative atomic mass?
Ar= total mass of atoms/ total number of atoms let's say there are two isotopes -the formula would be ar= (mass of isotope 1× % of isotope 1) + (mass of isotope 2 x % isotope 2)/100
33
The table shows the mass numbers and abundances of naturally occurring copper isotopes. Mass number Abundance 63 69% 65 31% Calculate the relative atomic mass of copper. Give your answer to 1 decimal place.
(69x63) + (31 x65) / (69 +31) 63.62 63.6