Chapter 2 - Atoms, Ions and Compounds Flashcards

Atomic structure and isotopes, Relative mass and Formulae and equations

1
Q

What makes up the nucleus?

A

Protons and neutrons

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2
Q

What occupies the region around the nucleus?

A

Electrons

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3
Q

How are electrons arranged?

A

In shells around the nucleus

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4
Q

What is the charge of a proton?

A

+1

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5
Q

What is the charge of an electron?

A

-1

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6
Q

What charge does a neutron have?

A

0

It is neutral

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7
Q

Why do atoms have no overall charge?

A

The same number of electrons and protons so the charges cancel out.

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8
Q

What does atomic number represent?

A

The number of protons.

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9
Q

What are isotopes?

A

Atoms of the same element with the same number of protons but with different numbers of neutrons.

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10
Q

What does mass number represent?

A

The number of protons and neutrons.

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11
Q

Do isotopes react differently?

A

No, because chemical reactions involve electrons, not neutrons.

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12
Q

What is an ion?

A

A charged atom. Where the number of electrons and the number of protons differ.

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13
Q

What are cations?

A

Positive ions, atoms with fewer electrons than protons.

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14
Q

What are anions?

A

Negative ions, atoms with more electrons than protons.

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15
Q

What is relative isotopic mass?

A

The mass of an isotope relative to 1/12th of the mass of an atom of carbon-12.

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16
Q

What is relative atomic mass?

A

The weighted mean mass of an atom of an element relative to 1/12th of the mass of an atom of carbon-12.

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17
Q

How are percentage abundances of the isotopes in a sample of an element found?

A

Experimentally using a mass spectrometer.

18
Q

What do atoms of metals on the left of the periodic table tend to do with electrons?

A

Lose them to form cations.

19
Q

What do atoms of non-metals on the right of the periodic table tend to do with electrons?

A

Gain them to form anions.

20
Q

What is a binary compound?

A

A compound containing only two elements.

21
Q

What are polyatomic ions?

A

Ions contain atoms of more than one element bonded together

22
Q

What is the structure and charge of an ammonium ion?

A

NH(4)

1+

23
Q

What is the structure and charge of a hydroxide ion?

A

OH

1-

24
Q

What is the structure and charge of a nitrate ion?

A

NO(3)

1-

25
Q

What is the structure and charge of a nitrite ion?

A

NO(2)

1-

26
Q

What is the structure and charge of a hydrogencarbonate ion?

A

HCO(3)

1-

27
Q

What is the structure and charge of a manganate(VII) ion?

A

MnO(4)

1-

28
Q

What is the structure and charge of a carbonate ion?

A

CO(3)

2-

29
Q

What is the structure and charge of a sulfate ion?

A

SO(4)

2-

30
Q

What is the structure and charge of a sulfite ion?

A

SO(3)

2-

31
Q

What is the structure and charge of a dichromate(VI) ion?

A

Cr(2)O(7)

2-

32
Q

What is the structure and charge of a phosphate ion?

A

PO(4)

3-

33
Q

What is the structure and charge of a zinc ion?

A

Zn

2+

34
Q

What is the structure and charge of a sodium ion?

A

Na

1+

35
Q

What is the structure and charge of a halide ion?

A

F/Cl/Br/I/At

1-

36
Q

What is the structure and charge of an aluminium ion?

A

Al

3+

37
Q

What must an ionic compound have?

A

An overall charge of zero.

38
Q

What is a diatomic molecule?

A

Two atoms of the same element bonded together.

39
Q

Do covalent compounds contain ions?

A

No, they do not.

40
Q

Where are state symbols shown in chemical equations?

A

In subscript in brackets after a formula.