atomic structure Flashcards

1
Q

What are atoms?

A

Atoms are the smallest part of an element that can exist.

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2
Q

What do chemical symbols represent?

A

Chemical symbols represent an atom of an element.

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3
Q

How are compounds formed?

A

Compounds are formed from elements by chemical reactions.

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4
Q

What do chemical reactions involve?

A

Chemical reactions involve the formation of one or more new substances and often an energy change.

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5
Q

What do compounds contain?

A

Compounds contain two or more elements chemically combined in fixed proportions.

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6
Q

What is a mixture?

A

A mixture consists of two or more elements or compounds not chemically combined together.

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7
Q

How do the chemical properties of substances in a mixture compare to those in a compound?

A

The chemical properties of each substance in the mixture are unchanged, unlike in a compound.

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8
Q

How can mixtures be separated?

A

Mixtures can be separated by filtration, crystallisation, simple distillation, fractional distillation, and chromatography.

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9
Q

What was the first thought about the structure of atoms?

A

Atoms were thought to be tiny spheres that could not be divided.

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10
Q

How are elements arranged in the periodic table?

A

Elements are arranged in order of atomic (proton) number.

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11
Q

What is the significance of groups in the periodic table?

A

Elements with similar properties are found in the same columns, known as groups.

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12
Q

What do elements in the same periodic group have in common?

A

They have the same amount of electrons in their outer shell.

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13
Q

What model was proposed after the discovery of the electron?

A

The plum pudding model was proposed, where the atom is a ball of positive charge with negative electrons embedded in it.

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14
Q

What did the alpha particle scattering experiment conclude?

A

The experiment concluded that the mass of an atom was concentrated at the center (nucleus) and that the nucleus was charged.

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15
Q

Who ordered the periodic table by atomic weight?

A

John Newlands ordered his table by atomic weight.

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16
Q

What was the setup of the alpha particle scattering experiment?

A

A beam of alpha particles was aimed at very thin gold foil, and their passage through was detected.

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17
Q

What is the ‘law of octaves’ proposed by John Newlands?

A

Similar properties occur every eighth element.

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18
Q

What was observed during the alpha particle scattering experiment?

A

Some alpha particles emerged from the foil at different angles, and some even came straight back.

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19
Q

Why were the alpha particles deflected during the experiment?

A

The positively charged alpha particles were being repelled and deflected by a small concentration of positive charge in the atom (nucleus).

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20
Q

What limitation did Newlands’ periodic table have?

A

It broke down after calcium.

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21
Q

How did Mendeleev organize his periodic table?

A

Mendeleev ordered his table by atomic mass, but not always strictly.

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22
Q

Who suggested that electrons orbit the nucleus at specific distances?

A

Neil Bohr suggested that electrons orbit the nucleus at specific distances.

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23
Q

What did later experiments reveal about the nucleus?

A

Later experiments revealed that the positive charge of any nucleus could be subdivided into smaller particles, each having the same amount of positive charge (protons).

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24
Q

Why did Mendeleev leave gaps in his periodic table?

A

He left gaps for elements that he thought had not been discovered yet.

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25
Q

Why is the table called a periodic table?

A

Because similar properties occur at regular intervals.

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26
Q

Who provided evidence for the existence of neutrons?

A

James Chadwick provided evidence to show the existence of neutrons within the nucleus.

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27
Q

What was discovered that filled the gaps in Mendeleev’s periodic table?

A

Elements with properties predicted by Mendeleev were discovered.

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28
Q

How did knowledge of isotopes affect the periodic table?

A

It explained why the order based on atomic weights was not always correct.

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29
Q

What is the atomic number?

A

The atomic number is the number of protons in an atom of an element.

30
Q

What discovery in the early 20th century changed the ordering of elements?

A

The discovery of electrons, protons, and neutrons led to ordering by atomic (proton) number.

31
Q

Where are metals typically found in the periodic table?

A

Metals are found to the left and towards the bottom of the periodic table.

32
Q

What are non-metals defined as in the periodic table?

A

Non-metals are elements that do not form positive ions.

33
Q

What is the relative charge of a proton?

A

The relative charge of a proton is +1.

34
Q

What is the relative charge of a neutron?

A

The relative charge of a neutron is 0.

35
Q

Where are non-metals typically found in the periodic table?

A

Non-metals are found towards the right and top of the periodic table.

36
Q

What is the relative charge of an electron?

A

The relative charge of an electron is -1.

37
Q

What characteristic properties do alkali metals have?

A

They have a single electron in their outer shell.

38
Q

What is the overall charge of an atom?

A

An atom has an overall charge of 0, so the number of protons equals the number of electrons.

39
Q

What is the approximate radius of an atom?

A

The radius of an atom is about 0.1 nm.

40
Q

How do alkali metals react with water?

A

They react vigorously with water to create an alkaline solution and hydrogen.

41
Q

How does the radius of a nucleus compare to that of an atom?

A

The radius of a nucleus is less than 1/10,000 of that of the atom.

42
Q

What do alkali metals produce when they react with oxygen?

A

They all react with oxygen to create an oxide.

43
Q

What do alkali metals form when they react with chlorine?

A

They all react with chlorine to form a white precipitate.

44
Q

What does the mass of the nucleus represent?

A

The nucleus holds almost all of the mass of the atom.

45
Q

How do transition elements compare to group 1 elements in terms of hardness and strength?

A

Transition elements are harder and stronger.

46
Q

How does reactivity change among alkali metals in Group 1?

A

The reactivity of the elements increases going down the group.

47
Q

What is a notable exception regarding the melting points of transition elements?

A

Mercury has a lower melting point compared to other transition elements.

48
Q

What is the relative mass of a proton?

A

The relative mass of a proton is 1.

49
Q

How do transition elements react with oxygen and water compared to group 1 elements?

A

Transition elements are much less reactive and do not react as vigorously with oxygen or water.

50
Q

What is the relative mass of a neutron?

A

The relative mass of a neutron is 1.

51
Q

What is the mass number?

A

The mass number is the sum of the protons and neutrons in an atom.

52
Q

How many electrons do noble gases have in their outer shell?

A

Noble gases have 8 electrons in their outer shell, except helium, which has 2.

53
Q

Why are noble gases unreactive?

A

They have a stable arrangement of electrons with full outer shells.

54
Q

What are the properties of the transition element iron?

A

Good conductor, rusts easily in air, strong and ductile.

55
Q

How do the boiling points of noble gases change?

A

The boiling points increase with increasing relative atomic mass going down the group.

56
Q

What are isotopes?

A

Isotopes are atoms of the same element with different numbers of neutrons.

57
Q

What do halogens have in common regarding their outer shell electrons?

A

Halogens have seven electrons in their outer shell.

58
Q

What are the properties of the transition element cobalt?

A

Malleable, brittle, hard with a high melting point.

59
Q

How are atoms shown in the periodic table?

A

Atoms are shown in the periodic table by their relative atomic mass.

60
Q

How do halogens exist in nature?

A

Halogens exist as molecules made of pairs of atoms (e.g., Cl2).

61
Q

What are the properties of the transition element nickel?

A

Hard, malleable and ductile, fairly good conductor of heat and electricity.

62
Q

What is relative atomic mass?

A

Relative atomic mass is an average value that takes account of the abundance of the isotopes of the element.

63
Q

What type of compounds do halogens form when they react with metals?

A

They form ionic compounds where the halide ion carries a -1 charge.

64
Q

What are the properties of the transition element copper?

A

Highly ductile and conductive, malleable and soft.

65
Q

What type of compounds do halogens form when they react with nonmetals?

A

They form covalent compounds, where there is a shared pair of electrons.

66
Q

What is a typical property of transition elements regarding their ions?

A

They have ions with many different charges.

67
Q

How do the properties of halogens change down the group?

A

Relative molecular mass, melting point, and boiling point all increase down the group.

68
Q

What is a characteristic of compounds formed by transition elements?

A

They form coloured compounds.

69
Q

How does reactivity change among halogens in Group 7?

A

Reactivity decreases down the group.

70
Q

Why does reactivity decrease down the group for halogens?

A

Halogens react by gaining an electron, and the number of electron shells increases down the group.

71
Q

Why are transition elements useful as catalysts?

A

They facilitate chemical reactions without being consumed.