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Edexcel Chemistry GCSE > The periodic table > Flashcards

The periodic table Flashcards

Key concepts in chemistry

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1
Q

Abundance

Definition

A

If there is a lot of something, it is described as being abundant.

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2
Q

Atom

definition

A

The smallest part of an element that can exist.

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3
Q

Atomic number

definition

A

The number of protons and neutrons in the nucleus of an atom. Also called the atomic proton number.

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4
Q

Chemical properties definition

A

A description of how a substance reacts with other substances. For example, flammability, pH, reaction with an acid, etc.

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5
Q

Compound

Definition

A

A substance formed by the chemical union of 2 or more elements.

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6
Q

Electron

definition

A

Subatomic particle with a negative charge and a negligible mass relative to protons and neutrons.

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7
Q

Electron arrangement configuration

Definition

A

The order electrons are arranged into between different energy levels(shells).

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8
Q

Element

definition

A

A substance made up of one type of atoms only.

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9
Q

Group
(periodic table)
Definition

A

A vertical column in the periodic table containing elements with similar chemical properties.

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10
Q

Isotope

Definition

A

Atoms of an element with the same number of protons and electrons but different numbers of neutrons.

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11
Q

Metal

Definition

A

Shiny element that is a good conductor of electricity and heat, and which forms basic oxides.

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12
Q

properties

Definition

A

The characteristics of something. In chemistry, chemical properties include the reactions a substance can take part in. Physical properties include colour and boiling point.

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13
Q

physical properties

Definition

A

A description of the appearance of a substance or how it acts without involving chemical reactions. For example, state, melting point, conductivity, etc.

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14
Q

periodic trend

definition

A

A pattern in chemical or physical properties of elements in the periodic table.

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15
Q

period

definition

A

A horizontal row in the periodic table.

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16
Q

nucleus

Definition

A

The central part of an atom. It contains protons and neutrons, and has most of the mass of the atom. The plural of nucleus is nuclei.

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17
Q

non-metal

Definition

A

Element that is a poor conductor of electricity and heat, and which forms acidic oxides.

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18
Q

proton

Definition

A

Subatomic particle with a positive charge and a relative mass of 1. The relative charge of a proton is +1.

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19
Q

relative atomic mass

Definition

A

The mean relative mass of the atoms of the different isotopes in an element. It is the number of times heavier an atom is than one-twelfth of a carbon-12 atom.

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20
Q

Who is Dmitri Mendeleev?

A

Like many scientists working at the end of the 19th-century the Russian chemist Dmitri Mendeleev (1834-1907) was looking for ways to organise the known elements. Mendeleev published his first periodic table of the elements in 1869.

21
Q

Features of Mendeleev’s tables

A

Mendeleev arranged the elements in order of increasing relative atomic mass. When he did this he noted that the chemical properties of the elements and their compounds showed a periodic trend. He then arranged the elements by putting those with similar properties below each other into groups

22
Q

Features of Mendeleev’s tables

To make his classification work Mendeleev made a few changes to his order:

A
  • he left gaps for yet to be discovered elements

- he switched the order of a few elements to keep the groups consistent

23
Q

Features of Mendeleev’s tables

Predictions using gaps

A

Mendeleev left gaps in his table to place elements not known at the time. By looking at the chemical properties and physical properties of the elements next to a gap, he could also predict the properties of these undiscovered elements. For example, Mendeleev predicted the existence of ‘eka-silicon’, which would fit into a gap next to silicon. The element germanium was discovered later. Its properties were found to be similar to the predicted ones and confirmed Mendeleev’s periodic table.

24
Q

Features of Mendeleev’s tables

Pair reversals

A

Iodine has a lower relative atomic mass than tellurium. So iodine should be placed before tellurium in Mendeleev’s tables. However, iodine has similar chemical properties to chlorine and bromine. To make iodine line up with chlorine and bromine in his table, Mendeleev swapped the positions of iodine and tellurium.

25
Q

How are elements arranged in a modern periodic table?

A

In the modern periodic table, the elements are arranged according to their atomic number

26
Q

In the periodic table the elements are arranged into:

A

rows, called periods, in order of increasing atomic number

vertical columns, called groups, where the elements have similar properties

27
Q

In the periodic table, what are periods?

A

Rows, in order of increasing atomic number

28
Q

In the period table, what are groups?

A

Vertical columns, the elements have similar properties

29
Q

Metals and non-metals in the periodic table

A

The metal elements are found on the left hand side of the periodic table, and the non-metal elements are found on the right. Imagine a zig-zag line, starting at B-Al-Si, separating metals from non-metals.

30
Q

Mendeleev

Isotopes

A

Mendeleev did not know about isotopes, but their existence is an explanation for pair reversals in his table.

31
Q

The positions of iodine and tellurium were reversed in Mendeleev’s table because:

A
  • iodine has one naturally occurring isotope, iodine-127

- the most abundant tellurium isotopes are tellurium-128 and tellurium-130

32
Q

What is the way in which electrons are arranged in an atom called?

A

Electron configuration

33
Q

Predicting an electronic configuration

A

The electronic configuration of an atom can be predicted from its atomic number.

34
Q

How is the electronic configuration feature: Number or numbers of circles linked to the periodic table?

A

Link to the periodic table:

Period number

35
Q

How is the electronic configuration feature: Number of electrons in outermost shell linked to the periodic table?

A

Link to the periodic table:

Group number

36
Q

How is the electronic configuration feature: Total number of electrons in all shells linked to the periodic table?

A

Link to the periodic table:

Atomic number

37
Q

The electronic configuration of sodium is (2.8.1)

List it’s period, group and atomic number

A

sodium, Na:

  • is in period 3
  • is in group 1
  • has an atomic number of (2 + 8 + 1) = 11
38
Q

Which electrons meet and interact when atoms collide and react?

A

When atoms collide and react, it is the outer electrons that meet and interact.

39
Q

Elements in the same group have similar, what?

why?

A

Elements in the same group have similar chemical properties because they have the same number of electrons in their outer shell.

40
Q

What order did Mendeleev place the elements in to form his first periodic table?

A

Mendeleev placed the elements in order of increasing atomic mass.

41
Q

How are the elements arranged in the modern periodic table?

A

In the modern periodic table the elements are arranged in order of increasing atomic number.

42
Q

Why did Mendeleev leave gaps in his periodic table?

A

Mendeleev realised that there were still some elements to be discovered. When the elements were discovered their properties matched the predicted properties.

43
Q

What is the electron arrangement of an element with an atomic number of 16?

A

2.8.6

44
Q

What name is given to the horizontal rows in the periodic table?

A

Periods

45
Q

Where is the element with the electron arrangement: 2.8.8.2 found in the periodic table?

A

The element is found in period 4 and group 2

46
Q

Which part of the atomic structure has most effect on the chemical properties and reactions of an element?

A

The outer electron shell

47
Q

What changes in atomic structure occur as you move from left to right along the horizontal rows in the periodic table?

A

The number of protons in the nucleus increases by one.

48
Q

What changes in atomic structure occur as you move from top to bottom along vertical rows?

A

The number of electron shells increases by one each time you go down into the next period.

Edexcel Chemistry GCSE (10 decks)

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