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Harvey's maths lessons > Periodic Table > Flashcards

Periodic Table Flashcards

1
Q

What is an atom?

A

The smallest part of an element that can exist.

Atoms are the basic building blocks of matter.

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2
Q

Describe Dalton’s model of the atom.

A

Atoms as solid spheres that cannot be divided into smaller parts.

Dalton proposed that atoms are indivisible and maintain their identity in chemical reactions.

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3
Q

What is an element?

A

A substance made of one type of atom.
E.g., oxygen = O2, iron = Fe.

Elements are pure substances that cannot be broken down into simpler substances.

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4
Q

What is a molecule?

A

A particle made of two or more atoms joined together.
E.g., oxygen = O3, water = H2O.

Molecules can consist of the same or different types of atoms.

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5
Q

What is a diatomic molecule?

A

A molecule that consists of two atoms, often the same.
E.g., O2, Cl2.

Diatomic molecules are important in various chemical reactions.

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6
Q

What is a chemical symbol?

A

A one or two universal letter code of each element.

Chemical symbols are used to represent elements in chemical formulas.

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7
Q

Where are chemical symbols of elements found?

A

In the periodic table.

The periodic table organizes elements based on their properties.

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8
Q

What is a compound?

A

A substance made of more than one type of atom chemically joined together.
E.g., water = H2O, carbon dioxide = CO2.

Compounds have different properties than the elements that make them up.

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9
Q

What is a chemical formula?

A

A formula that shows the number and type of atoms present in a molecule.

Chemical formulas provide essential information about the composition of compounds.

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10
Q

What do the compound endings ‘ide’ and ‘ate’ mean?

A

1) ide - a compound of only the named substances.
2) ate - a compound of the named substances and oxygen.

These endings help identify the composition of chemical compounds.

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11
Q

What is a physical change?

A

Changes of state as no new substances are made.

Physical changes include changes in state, shape, or size without altering the substance’s composition.

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12
Q

What is a chemical change (Chemical reaction)?

A

When atoms rearrange to make new substances.

Chemical changes involve breaking and forming bonds between atoms.

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13
Q

Where do we find metals in the periodic table?

A

On the left.

Metals are typically located on the left side of the periodic table and are characterized by specific physical properties.

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14
Q

Where do we find non-metals on the periodic table?

A

On the right.

Non-metals are found on the right side of the periodic table and have distinct properties compared to metals.

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15
Q

Who designed the modern periodic table?

A

Mendeleev.

Mendeleev organized elements based on atomic mass and properties, leading to the development of the periodic table.

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16
Q

What are the groups in the periodic table?

A

Columns.

Groups contain elements with similar chemical properties.

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17
Q

What are the rows called in the periodic table?

A

Periods.

Periods indicate the energy levels of the electrons in the atoms.

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18
Q

What are the physical properties of most metals?

A
  • Good conductors of electricity
  • Good conductors of heat
  • Shiny
  • High density (heavy for its size)
  • Malleable (can be hammered)
  • Sonorous (makes a ringing sound when hit)
  • Ductile (can be pulled into wires)
  • High melting points (except mercury)
  • Hard

Metals exhibit these characteristics due to their atomic structure.

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19
Q

What are the physical properties of non-metals?

A
  • Poor conductors of electricity
  • Poor conductors of heat
  • Dull
  • Low density (light for its size)
  • Brittle (breaks easily)
  • Non-sonorous (no ringing sound when hit)
  • Low melting points

Non-metals have distinct properties that differentiate them from metals.

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20
Q

What is the formula to calculate the relative atomic mass of an element with isotopes?

A

((isotope 1 mass x abundance) + (isotope 2 mass x abundance)) ÷ 100

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21
Q

How do you calculate the relative atomic mass of carbon with isotopes carbon-14 and carbon-12?

A

For carbon: ((14 × 20) + (12 × 80)) ÷ 100 = 12.4

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22
Q

What do electrons occupy in an atom?

A

Electrons occupy the lowest available energy levels (the shells closest to the central nucleus).

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23
Q

What does the electronic structure of an atom indicate?

A

The electronic structure tells you how many electrons are in each shell.

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24
Q

What is the electronic structure of sodium?

A

2, 8, 1

Sodium has 2 electrons in shell 1, 8 in shell 2, and 1 in shell 3.

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25
Q

What are atoms?

A

Atoms make up all substances and are the smallest part of an element that can exist

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26
Q

What do chemical symbols represent?

A

Chemical symbols represent an atom of an element; e.g., Na represents an atom of sodium

27
Q

How are compounds formed?

A

Compounds are formed from elements by chemical reactions

28
Q

What do compounds contain?

A

Compounds contain two or more elements chemically combined in fixed proportions

29
Q

Give an example of a compound and its composition.

A

HCl is a compound containing 1 atom of hydrogen and 1 of chlorine per molecule

30
Q

How can compounds be separated into elements?

A

Compounds can only be separated into elements by chemical reactions

31
Q

What is a mixture?

A

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

32
Q

What happens to the chemical properties of substances in a mixture?

A

The chemical properties of each substance in the mixture are unchanged

33
Q

How can mixtures be separated?

A

Mixtures can be separated by:
* filtration
* crystallisation
* simple distillation
* fractional distillation
* chromatography

34
Q

What distinguishes the separation of mixtures from compounds?

A

Separation of mixtures involves physical processes, so no new substances are made

35
Q

What was the first model of the atom?

A

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

36
Q

What is the plum pudding model?

A

The plum pudding model describes the atom as a ball of positive charge with negative electrons embedded in it

37
Q

What conclusion was drawn from the alpha particle scattering experiment?

A

The mass of an atom was concentrated at the centre (nucleus) and that the nucleus was charged

38
Q

Describe the alpha particle scattering experiment.

A

A beam of alpha particles was aimed at very thin gold foil; some particles were deflected at different angles and some came straight back

39
Q

What did the scattering experiment reveal about the nucleus?

A

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

40
Q

What did Neil Bohr suggest about electrons?

A

Neil Bohr suggested that electrons orbit the nucleus at specific distances

41
Q

True or False: A mixture can only be separated by chemical reactions.

A

False

42
Q

Fill in the blank: Compounds can only be separated into elements by _______.

A

chemical reactions

43
Q

What is the positive charge of any nucleus subdivided into?

A

Whole number of smaller particles called protons

44
Q

Who provided the evidence for the existence of neutrons?

A

James Chadwick

45
Q

What is the atomic number?

A

The number of protons in an atom of an element

46
Q

Do all atoms of a particular element have the same number of protons?

A

Yes

47
Q

What is the relative charge of a proton?

A

+1

48
Q

What is the relative charge of a neutron?

A

0

49
Q

What is the relative charge of an electron?

A

-1

50
Q

What must be true for an atom to have an overall charge of 0?

A

Number of protons = number of electrons

51
Q

What is the approximate radius of an atom?

A

About 0.1 nm

52
Q

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

A

Less than 1/10,000 of that of the atom

53
Q

What is the mass number?

A

The sum of the protons and neutrons in an atom

54
Q

What are isotopes?

A

Atoms of the same element with different numbers of neutrons

55
Q

What does the mass number indicate in the periodic table?

A

Total number of protons and neutrons

56
Q

If an atom has a mass number of 19 and 9 protons, how many neutrons does it have?

A

10 neutrons

57
Q

What is relative atomic mass?

A

An average value that takes account of the abundance of the isotopes of the element

58
Q

What does the atomic number indicate?

A

The number of protons in an atom

59
Q

Fill in the blank: Atoms are very small, with a radius of about _______.

A

0.1 nm

60
Q

True or False: An electron has a relative mass of 1.

A

False

61
Q

What is the relative mass of a proton?

A

1

62
Q

What is the relative mass of a neutron?

A

1

63
Q

What is the relative mass of an electron?

A

Very small

Harvey's maths lessons (5 decks)

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