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Science > Science y10 > Flashcards

Science y10 Flashcards

1
Q

What is an isotope?

A

Isotopes are atoms of the same element with different mass numbers due to
different numbers of neutrons in the nucleus.

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2
Q

What did Democritus think of atoms in 400 BC?

A

Before the discovery of the electron, atoms were
thought to be tiny spheres that could not be
further divided – Democritus called them the
‘smallest piece’ of matter

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3
Q

What did John Dalton discover in 1803?

A

John Dalton also stated that matter is made of tiny particles called atoms but
thought there could be different types. He suggested they could combine to form
compounds

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4
Q

What did John Dalton start in 1803?

A

He began to put these atoms into a table.The beginning of our modern periodic table.

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5
Q

What did J.J Thompson in 1904?

A

The discovery of the electron by Joseph (JJ) Thomson led to the plum pudding
model of the atom.

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6
Q

What is the plum pudding model?

A

The plum pudding model suggested that the
atom is a ball of positive charge with
negative electrons embedded in it

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7
Q

What did Ernest Rutherford discover in 1905?

A

The results from the alpha particle scattering experiment performed by Ernest
Rutherford, as well as Geiger and Marsden, showed that most of the mass of
the atom was concentrated at the centre of the atom (the nucleus), which was
charged
This was the beginning of the
nuclear model.

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8
Q

What did Niels Bohr in 1922?

A

Niels Bohr further adapted the nuclear model when his
calculations and experiments proved the electrons
orbited the nucleus at specific distances (energy
levels)

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9
Q

What did James Chadwick do in 1932?

A

James Chadwick’s experimental work provided the
evidence to show the existence of neutrons in the
nucleus

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10
Q

What is the nuclear model?

A

The nuclear model proposed by Rutherford in 1911 pictures the atom as a heavy, positively-charged nucleus, around which much lighter, negatively-charged electrons circulate, much like planets in the Solar system.

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11
Q

What is the atomic number?

A

The number of protons and electrons in an atom of an element.

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12
Q

What is a mass number?

A

The number of protons and neutrons in an atom of an element.

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13
Q

How do calculate neutrons?

A

Number of neutrons = mass number - atomic number

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14
Q

Where are electrons found in an atom?

A

In energy levels orbiting the
nucleus

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15
Q

How many electrons can be held in the first energy level?

A

Two

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16
Q

How many electrons can be held in the second energy level?

A

Eight

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17
Q

How can you calculate the number of electrons in an atom?

A

In an atom the number of electrons is equal to the number of protons, which
is the atomic number

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18
Q

State (in numbers) the electronic configuration of an oxygen atom

A

2,6

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19
Q

what can atoms do to gain a full outer shell?

A

Atoms can lose or gain electrons to achieve a full outer
shell

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20
Q

What are gained or lost electrons called?

A

Atoms that have gained or lost electrons are called ions

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21
Q

How do metals form positive ions?

A

Metal atoms lose electrons to form positive
ions

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22
Q

How do metals make negative ions?

A

Non-metal atoms gain electrons to form
negative ions

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23
Q

What type of elements form negative ions?

A

Non-metals

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24
Q

What type of elements form positive ions?

A

Metals

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25
Q

How are positive ions formed?

A

Atoms lose electrons

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26
Q

How are negative ions formed?

A

Atoms gain electrons

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27
Q

Why are atoms considered electrically neutral?

A

Atoms have equal numbers of protons, which are positively charged and
electrons, which are negatively charged. This means that the charges cancel each
other out.

28
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

29
Q

What is the relative atomic mass number?

A

(mass number x abundance)+(mass number x abundance)

30
Q

What are elements in group 0 called?

A

Elements in Group 0 of the periodic table are called the noble gases

31
Q

What is the scientific word for unreactive?

A

inert

32
Q

How does the melting
point change as you
move down the noble
gases group?

A

The melting
point increases as
you move down the
noble gases group.

33
Q

Explain why the Noble Gases are described as having stable electronic
configurations.

A

They have a full outer shell

34
Q

Explain the difference between an atom being stable and an atom being
electrically neutral.

A

If an atom has a full outer shell this means it is stable.

If an atom has the same number of positive protons and
negative electrons this means that it is electrically neutral

All atoms are electrically neutral but not all atoms are stable.

35
Q

What is the subatomic particle discovered by James Chadwick.

A

The neutron

36
Q

What are the names given to columns and rows of the Periodic Table?

A

Columns are called groups and rows are called periods.

37
Q

How is the periodic table arranged?

A

Elements are arranged in the Periodic
Table in order of increasing atomic
(proton) number

38
Q

What are the properties of metals?

A

Most metals have high melting points, are good conductors of heat, good
conductors of electricity, malleable and ductile.

39
Q

Why is the periodic table called the periodic table?

A

It is called the Periodic Table because similar properties occur at regular
intervals. The word for this is periodicity.

40
Q

What is similar about the electrons of elements in each group?

A

Elements in the same group have the
same number of electrons in their
outer shell, which gives them similar
chemical properties

41
Q

Why did Mendeleev leave gaps in his Periodic Table?

A

He left gaps for elements he thought had not yet been discovered so they could fit
in the groups with elements that have similar properties.

42
Q

Where are the Alkali metals found on the Periodic Table?

A

Group 1

43
Q

why are alkali metals stored in oil

A

To minimize contact with oxygen and water

44
Q

What gas is produced in the reaction between the Alkali metals and water?

A

hydrogen

45
Q

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

A

hey have the same number of electrons in their outer shells, which gives them similar properties.

46
Q

What are elements in group 7 called?

A

Elements in Group 7 of the Periodic Table are called the Halogens

47
Q

How many electrons do group 7 elements have in their outer shells?

A

Halogens all have 7 electrons in their outer shell so have similar chemical properties

48
Q

What is the reactivity like in group 7?

A

In group 7, the further down the group an element is, the higher its melting point and boiling point. This is because, going down group 7:

the molecules become larger
The forces between the molecules become stronger
more energy is needed to overcome these forces

49
Q

How do halogens get a stable electronic configuration?

A

The halogens need to attract one negatively charged electron to have a stable electronic configuration.

50
Q

What type of elements does ionic bonding occur between?

A

Metals and non-metals

51
Q

What is a covalent bond?

A

A shared pair of electrons between two non-metal atoms

52
Q

What is an ion?

A

An ion is a charged particle, or group of particles

53
Q

When does ionic bonding occur?

A

Ionic bonding occurs in compounds formed from metals combined with non-metals.

54
Q

State the charge of electrons.

A

-1

55
Q

What are some properties of ionic substances?

A

Ionic substances

conduct electricity when molten or in solution.

are hard solids, with high melting and boiling points.

form crystalline structures

56
Q

What is the structure of ionic substances like?

A

Ionic substances

have a giant lattice structure, also called an
ionic lattice

have a regular, repeating pattern of
oppositely charged ions

are held together by strong electrostatic forces
of attraction (also called ionic bonds)

57
Q

Why do ionic substances have high melting and boiling points?

A

..due to strong electrostatic forces of
attraction between oppositely charged
ions. These require large amounts of
energy to overcome.

58
Q

Why can’t ionic substances conduct electricity in solids?

A

because the ions are fixed in position

59
Q

Why can ionic substances conduct electricity in molten and liquid form?

A

..because the ions are free to move and
carry the charge

60
Q

Why do ionic substances form hard crystalline substances?

A

..because the ions are tightly packed in a
regular, repeating structure called an
ionic lattice

61
Q

What is covalent bonding?

A

Covalent bonding occurs where two or more non-metal atoms share
pairs of electrons in order to achieve a stable electronic configuration

62
Q

What are the properties of simple covalent structures?

A

have low melting
and boiling points

are liquid or gas at
room temperature

do not conduct
electricity

63
Q

What are properties of giant covalent substances?

A

have high melting
and boiling points

are solid at room
temperature

may conduct
electricity

64
Q

Why do simple covalent substances have low melting points?

A

..they have weak intermolecular forces of
attraction between the molecules. These require
little energy to overcome and melt or boil the
substance.

65
Q

Why cant simple covalent substances conduct electricity?

A

..because the molecules are neutral (no charge),
they do not have any free electrons or ions to
carry a charge.

66
Q
A

Science (2 decks)

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