ATOMS AND PERIODIC TABLE Flashcards

1
Q

Explain why atoms have an overall neutral charge

A

Protons are positive and electrons are negative
Atoms have equal numbers of protons and electrons
So the charges sum to zero

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2
Q

Describe at least 2 features of the Bohr model of the atom

A

Electrons orbit the nucleus at specific distances
Atoms have a positive nucleus
Mass is concentrated in the nucleus
Atoms are mostly empty space

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3
Q

Explain why Mendeleev left gaps in the periodic table

A

For undiscovered elements

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4
Q

State the relative charges of the 3 subatomic particles

A

Proton = +1
Neutron = 0
Electron = -1

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5
Q

State the overall charge of an atom

A

0

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6
Q

Describe the information about the electronic structure provided by an element’s period in the periodic table

A

How many shells an atom has

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7
Q

Name 2 characteristics of atoms proved by the gold foil experiment

A

The mass of an atom is concentrated in the nucleus
The nucleus has a positive charge

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8
Q

Give 2 ways in which elements are ordered in the modern periodic table

A

First by their atomic number, then in groups based on their properties

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9
Q

Give the word for the percentage of atoms in a sample that are a particular isotope

A

Abundance

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10
Q

Electronic configuration of sulfur

A

2.8.6

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11
Q

State the relative masses of the 3 subatomic particles

A

Proton = 1
Neutron = 1
Electron = very small p

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12
Q

In the modern atomic model, name the subatomic particles found in the nucleus

A

Protons and neutrons

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13
Q

Name the 4 main historical models of the atom in chronological order

A

Dalton, Plum Pudding, Nuclear , Bohr

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14
Q

Before Mendeleev, explain how scientists ordered the elements

A

By their Atomic weights

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15
Q

Explain why Mendeleev’s periodic table was eventually accepted by other scientists

A

Elements were discovered which filled the gaps and matched the properties he predicted

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16
Q

Describe the difference between mass number and relative atomic mass

A

Mass number is the number of protons and neutrons in one atom
Relative atomic mass is an average value that takes account of isotopes

17
Q

Define isotopes

A

Atoms of the same element with different numbers of neutrons

18
Q

Diagrams

A

Diagrams on iPad