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chemistry > Chemical Changes And Structure #2: Periodic Table & Atomic Structure > Flashcards

Chemical Changes And Structure #2: Periodic Table & Atomic Structure Flashcards

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1
Q

How are elements in the periodic table arranged?

A

In order of increasing atomic number

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2
Q

What can the periodic table be used to determine?

A

Whether an element is a metal or a non-metal

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3
Q

What can we do with the electron arrangement of the first 20 elements?

A

Write them

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4
Q

What does an atom have?

A

A nucleus

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5
Q

How many types of atom are in each element?

A

1

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6
Q

What does a nucleus contain?

A
  • protons and neutrons
  • electrons that orbit the nucleus
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7
Q

What is the charge of a proton?

A

One-positive

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8
Q

What is the charge of a neutron?

A

Neutral

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9
Q

What is the charge of an electron?

A

One-negative

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10
Q

What is the relative weight / amu of a proton?

A

1

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11
Q

What is the relative weight / amu of an electron?

A

Almost zero

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12
Q

What is the relative weight / amu of a neutron?

A

1

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13
Q

Where is the proton?

A

In the nucleus

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14
Q

Where is the neutron?

A

In the nucleus

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15
Q

Where is the electron? Why?

A

Orbiting the nucleus, it is negatively charged and so attracted to the positive nucleus - opposites attract

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16
Q

What is relative weight?

A

Atomic mass (amu)

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17
Q

Atomic number =

A

Number of protons , number of electrons

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18
Q

Mass number =

A

Number of protons and neutrons

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19
Q

How do we find the number of neutrons?

A

Mass number - atomic number

20
Q

What is the charge of the nucleus?

A

Positive, because it’s positively and neutrally charged

21
Q

What is nuclide notation used to show?

A

The atomic number, mass number (and charge) of atoms (ions) from which the number of protons, neutrons, and electrons can be determined

22
Q

What is an isotope? (test question)

A

Atoms of the same element that have the same atomic number but a different mass number

23
Q

Isotopes have the exact same…

A

Chemical properties as other atoms

24
Q

What does it mean that isotopes have a different mass number?

A

Of the 118 atoms, some are heavier because they have a different amount of neutrons and so different mass numbers.

25
Q

If atoms of the same element can have a different amount of neutrons, what else must be different?

A

Their mass

26
Q

How do chemists use an average mass of the atoms in an element for calculations?

A

They take into account different isotopes and their relative abundance

27
Q

What do elements in a group in the periodic table have in common?

A

Similar chemical properties

28
Q

5 Properties of alkali metals

A
  • Very reactive
  • Soft
  • Stored under oil
  • Reaction with H20 = Alkaline solution
  • Reaction with oxygen = metal oxide
29
Q

4 properties of the transition metals

A
  • hard and dense
  • less reactive
  • used as catalysts
  • form coloured compounds
30
Q

5 properties of the halogens

A
  • diatomic elements
  • All toxic
  • flourine added to toothpaste to prevent decay
  • chlorine sterilises swimming pools
  • iodine treats wounds
31
Q

2 Properties of noble gases

A
  • not reactive at all
  • least reactive of all the elements
32
Q

Ways to remember how to work out nuclide notation

A

Atomic number = protons = electrons
Mass number = protons + neutrons
Neutrons = mass number - atomic number

33
Q

What does RAM take into account?

A

Different isotopes and their relative abundance

34
Q

Why do elements in a group have similar chemical properties?

A

They have the same number of outer electrons

35
Q

How many electrons can the first energy level hold?

A

2

36
Q

How many electrons can the 2nd and 3rd energy levels hold?

A

8 each

37
Q

How are elements arranged in periods?

A

In order of increasing atomic number

38
Q

When are ions formed?

A

When atoms gain or lose electrons

39
Q

What happens when an atom gains an electron?

A

It becomes a negatively charged ion

40
Q

What happens when an atom loses an electron?

A

It becomes a positively charged ion

41
Q

Non metals gain electrons to become…

A

negatively charged ions

42
Q

Metals lose electrons to become…

A

Positively charged ions

43
Q

What do atoms achieve by forming ions?

A

The same arrangement as the nearest noble gas

44
Q

Why are noble gases unreactive?

A

They have a stable outer electron arrangement

45
Q

Something to note about group 7

A

Reactive non-metals

46
Q

Something to note about Group 8

A

Un-reactive non-metals

chemistry (7 decks)

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