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GCSE Chemistry > C1 - Atomic Structure > Flashcards

C1 - Atomic Structure Flashcards

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1
Q

Atom

A

Smallest part of an element

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2
Q

Molecule

A

Two or more atoms, chemically bonded together.

e.g. O sub-script 2

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3
Q

Compound

A

A new substance made when ( two or more elements / two or more TYPES of atoms ) are chemically bonded together.

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4
Q

Mixture

A

When two or more substances are mixed together, but do not chemically react to make a new substance.

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5
Q

Element

A

A substance containing only one type of atom, and cannot be broken down into another substance.

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6
Q

Periodic Table

A

A chart containing all known elements, arranged according to their atomic mass.

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7
Q

Atomic Mass

A

The total number of protons and neutrons present in the nucleus of an element.

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8
Q

Atomic Number

A

The number of protons present in the nucleus of an element.

Also equals the number of electrons.

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9
Q

Ionic Bond

A

When two substances chemically bond as a result of their ions having opposite charges attracted to one another.

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10
Q

Covalent Bond

A

When two substances are chemically bonded by sharing electrons.

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11
Q

Shells

A

Where electrons are grouped in energy levels around the nucleus.

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12
Q

Group

A

A vertical column of the periodic table.

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13
Q

How to find the group of an element

A

The amount of electrons on an element’s outer-most shell corresponds to the periodic group number.

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14
Q

Units for Reference

A
  • 1 metre (m) = 1000 milimetres (mm)
  • 1 milimetre (mm) = 1000 micrometres (μm)
  • 1 micrometre (μm) = 1000 picometres (pm)
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15
Q

General rules of Standard Form

A

• 1 x 10^-3 … Move decimal point forward by 3 places.
= 0.001

• 1 x 10^3 … Move decimal point backwards by 3 places.
= 1000

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16
Q

How to find number of neutrons in an element

A

Mass Number - Atomic Number

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17
Q

( Mass Number / Atomic Mass ) Equation

A

Number of Protons + Number of Neutrons

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18
Q

Simplest group of hydrocarbons

A

Alkanes

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19
Q

What series of compounds are alkanes?

A

Homologous; group of compounds with similar properties.

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20
Q

How many bonds do alkanes have between their carbon atoms?

A

single bonds.

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21
Q

Alkanes are described as…

A

… Saturated hydrocarbons.

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22
Q

Relative Atomic Mass (Ar)

A

The little number to the top left of an element. It is the average of all isotopes of a given element, since they can vary in amount of electrons.

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23
Q

First 5 elements of the Periodic Table

A

Hydrogen, Helium, Lithium, Beryllium, Boron

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24
Q

Elements in Period 1

A

Helium. That’s all.

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25
Q

First 10 elements of the Periodic Table

A

Hydrogen, Helium, Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen, Fluorine, Neon.

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26
Q

First 15 elements of the Periodic Table?

A

Hydrogen, Helium, Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen, Fluorine, Neon, Sodium, Magnesium, Aluminium, Silicon, Phosphorus.

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27
Q

First 20 elements of the Periodic Table!

A

Hydrogen, Helium, Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen, Fluorine, Neon, Sodium, Magnesium, Aluminium, Silicon, Phosphorus, Sulfur, Chlorine, Argon, Potassium, Calcium.

28
Q

First 20 elements of the Periodic Table Symbols

A

H, He, Li, Be, B, C, N, O, F, Ne, Na, Mg, Al, Si, P, S, Cl, Ar, K, Ca

29
Q

Smallest part of an element

A

Atoms.

30
Q

Atom radius

A

0.1 nm , or 1 x 10^-10 m

31
Q

Avogadro’s Constant

A

6.022 x 10^23

32
Q

[True or False] An element contains only one type of atom.

A

True.

33
Q

Basic structure of an Atom

A

Electrons orbit the nucleus of an atom in shells. The nucleus is made from protons and neutrons.

There are the same amount of protons as there are electrons in an atom in an element.

34
Q

What is the significance of using chemical symbols in formulae and equations?

A

Scientists globally from any country can collaborate and work together without any language barriers, and therefore makes scientific endeavours easier.

35
Q

What electrical charge do protons, neutrons, and electrons have respectively?

A

Protons = +1

Neutrons = 0

Electrons = -1

It is important that you have the number 1.

36
Q

What atomic model is associated with John Dalton?

A

Solid Sphere model, at the start of the 19th century.

37
Q

Atomic model associated with JJ Thompson

A

Plum Pudding model, in 1897.

38
Q

Atomic model associated with Ernest Rutherford*

A

Nuclear model, around 1909.

  • Refer to alpha-scattering particle experiment.
39
Q

Atomic model associated with Niels Bohr

A

Planetary model, around 1913.

40
Q

Atomic model associated with James Chadwick

A

Quantum atomic model around 1940.

41
Q

John Dalton’s discovery

at the start of the 19th century

A

Recognised atoms of a particular element differ from other elements.

His theory stated:

  • Atoms are indivisible,
  • Those of a given element are identical,
  • and compounds are combinations of different types of atoms.
42
Q

JJ Thompson’s discovery in 1897

A

Discovered the electron.

The “Plum Pudding” model shows the atom composed of electrons, scattered throughout a spherical cloud of positive charge.

This ‘cloud’ concept is brought back by a later scientist.

43
Q

Ernest Rutherford’s discovery around 1909

A

His alpha-scattering particle experiment…

… Allowed for the discovery of a positive charge within the nucleus.

Particles of the same charge repel, thus he concluded on this basis for positive charges in the nucleus.

44
Q

Niels Bohr’s discovery around 1913

A

He modified Rutherford’s model and said electrons orbit the nucleus in shells of energy.

However, electrons could not take the place of values of energy between fixed energy levels.

45
Q

James Chadwick’s discovery around 1940

A

Discovered the neutron in the nucleus.

He bombarded beryllium atoms with alpha particles, similarly to Ernest Rutherford’s alpha-scattering particle experiment.

An unknown radiation was produced as a result.

Chadwick interpreted this radiation as being composed of particles with a neutral electrical charge and the approximate mass of a proton.

46
Q

Relative Mass of a Proton, a Neutron, and an Electron.

A

Proton = 1

Neutron = 1

Electron = 1/1836

47
Q

Sub-atomic particle symbol for Protons, Neutrons, and Electrons

A

Proton = p^+

Neutron = n^0

Electron = e^-

^ signifies the exponentiation.

48
Q

What does the Atomic Number tell us?

A

Number of protons, and also num of electrons in an atom.

The number of protons in an atom, sometimes called the proton number.

49
Q

Why don’t electrons ‘fall’ into the nucleus?

A

Well they do anyways.

Short and simple answer:

Electrons are trapped in electron shells that orbit the nucleus in layers, like an onion.

50
Q

General shell configuration of an atom

A

First shell = 2 electrons
Second shell = 8 electrons
Third shell = 8 electrons

Always start with the lowest available shell.

51
Q

Shorthand method of writing Shell structures of an atom

A

“2.8.8.2”

The first number indicated the lowest energy shell.

The full stops separates energy shells.

This would be the shell configuration for Calcium in the example.

52
Q

Isotope

A

Atoms which have different amounts of neutrons, but the same chemical properties.

ie same amount of protons and electrons.

53
Q

If an atom loses an electron …

A

The atom becomes positively charged: there is one proton that is not cancelled out.

54
Q

Ion

A

An atom that has gained or lost electrons and is now charged.

55
Q

What does the Atomic number dictate?

A

Dictates what element it is through its protons.

56
Q

What does the atomic number refer to?

A

The atomic number refers to the number of protons.

57
Q

How to tell what group an element is in

A

By the number of electrons an element has in their outer-most shell, using the configuration “2.8.8”.

58
Q

[True or False] Ions have a different group.

A

False.

Ions remain in their groups: ions just have an electrical charge.

59
Q

Atoms of the same element ___ have the same number of protons

A

Atoms of the same element ALWAYS have the same number of protons.

60
Q

[True or False] Atoms always have the same number of neutrons.

A

False. That’s why isotopes exist; isotopes have the same chemical properties between each other, but a different number of neutrons.

e.g. Carbon-12 and Carbon-13

61
Q

Isotopes are atoms with the same ___ ___, but not ___ ___.

A

Isotopes are atoms with the same ATOMIC NUMBER, but not ATOMIC MASS.

62
Q

Extra neutrons ___ makes the atom radioactive.

A

Sometimes.

63
Q

[True or False] Isotopes may also differ in physical properties.

A

True

64
Q

Isotopes ___ have the same chemical properties

A

Isotopes ALWAYS have the same chemical properties.

Due to same proton and electron configuration.

65
Q

Formula for relative atomic mass

A

relative atomic mass (Ar)

=

[ Sum of ( isotope abundance(%) x isotope mass number ) ]
/
Sum of abundances of all the isotopes.

66
Q

[Formula Example] Copper has two stable isotopes. Cu-63 has an abundance of 69.2% and Cu-65 has an abundance of 30.8%. Calculate the relative atomic of copper to 1 decimal place.

A 
Relative atomic mass = 
(69.2 x 63) + (30.8 x 65)
/
69.2 + 30.8
=
6361.6
/
100
=
63.616
=
63.6 (1dp)

GCSE Chemistry (2 decks)

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