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Chemistry > C3 Atoms, Elements Compounds > Flashcards

C3 Atoms, Elements Compounds Flashcards

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1
Q

Which group are the noble gases in the periodic table

A

Group 8

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2
Q

Why are the noble gases very unreactive

A

They have a full outershell, meaning they have the most stable electronic configuration

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3
Q

What is the most stable electron configuration

A

A full outer shell of electrons. Atoms react in order to gain a full outer shell of electron, so that they become more stable

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4
Q

Why are alloys harder than pure metals

A

Atoms in pure metals are in arranged uniform rows which can easily slide over each other making them malleable. Alloys contain different sized atoms which disort layers and are unable to slide. This makes it hard

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5
Q

Alloy

A

A mixture containing metals and another element

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6
Q

Covalent bond

A

A bond formed when two non metals share a pair of electrons

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7
Q

Isotopes

A

Atoms of an element with the same number of protons but a different number of neutrons. Ie same atomic number but different mass number

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8
Q

How are ions formed

A

Postive ions form when an atom loses electrons. Negative ions form when an atom gains electrons

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9
Q

What are ions

A

Atoms or groups of atoms with a positive or negative charge

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10
Q

What does atomic number represent

A

The number of protons in an atomic nucleus

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11
Q

What are cations ans anions

A

Cation-positive ion
Anion-negative ion

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12
Q

What types of elements are ionic bonds formed between

A

Between metals and non metals.
-Metals lose electrons to form positive ions.
- Non metals gain electrons to become negative ions.

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13
Q

Why do elements in the same group have similar chemical properties

A

Cuz they have the same number of electrons in the outer shell which determines how they react

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14
Q

How are elements arranged in the modern periodic table

A

In order of increasing atomic number. Elements with similar properties are in the same column

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15
Q

What does the mass of an atom mean?

A

The total number of protons and neutrons found in the nucleus of an atom

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16
Q

Why do atoms contain equal number of protons and electrons

A

Atoms are stable with no overall charge. There must be an equal number for the charges to balance

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17
Q

What are the relative charges of protons, neutrons and electrons

A

Proton: +1
Neutron: 0
Electron: -1

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18
Q

What does period(row) tell you about all the elements in that period

A

They have same number of electron shells. All elements in peiod 4 have 4 electron shells.

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19
Q

Why do ionic compounds have high melting and boiling points

A

Cuz they have strong electrostatic attraction between the oppositely charged particles. This requires a lot of energy to overcome meaning high melting and boiling points

20
Q

Desbribe the properties of a diamond

A

Very hard due to covalent bonding
Very high melting point due to covalent bonds

21
Q

Explain why metals are malleable

A

The ions are aaranged in regular uniform rows. These rows are able to slide over each other easily, making the metals malleable

22
Q

Difference between element and compound

A

An element is a substance made out of only 1 type if atom, whereas a compound is made up of two or more chemically combined elements

23
Q

Relative masses of protons, neutrons and electrons

A

Proton 1
Neutron 1
Electron 1/1836

24
Q

Two types of isotopes

A

Radioactive and non radioactive

25
Q

Solvent

A

A substance that dissolves to form a solution

26
Q

Concentration

A

A substance dissolved in a solution

27
Q

Mixture

A

Contains two or more elements or compounds that arent chemically combined

28
Q

Industrial use of radioactive isotopes

A

Smoke alarm tracker

29
Q

Explain the difference in melting and boiling points in the different types of covalent structured

A

Giant bonds-high boiling and melting point
Small bonds- low

30
Q

How are bonds formed between 1 and VII elements

A

G1 elements only lose 1 outer shell electron to form 1+ ions. Group VII elecment needs 1 ion in the outer shell that had 7 electrons. It gains 1- charge to form an ionic bond

31
Q

Non metal

A

Gain electrons to form negative ions. Top right in periodic table

32
Q

Metal

A

Lose electrons to form positive ions. Left side of the periodic table

33
Q

Why do atoms form covalent bonds

A

To obtain a more stable electron configuration

34
Q

Medical use of radioactive isotopes

A

Cancer treatment
Lung imaging

35
Q

Compare the solubility of ionic and covalent compounds

A

Ionic compounds are generally solubke in water, covalent compounds are insoulble in water

36
Q

What is brass? What are its uses

A

An alloy of copper and zinc.
Its hard and resistant to corrosion. It is used for decorative hardware such as plumbing fittings

37
Q

Name 2 giant structures formed from carbon atoms

A

Graphite
Diamond

38
Q

How are electrons arranged in an atom

A

In shells around the nucleus. The maz number of electrons in the first 3 shells is 2, 8,8

39
Q

How does electrical conductivity compare in the ionic and covalent compound

A

Covalent compounds dont have free compounds so they dont conduct electricity

Ionic compounds conduct electricity in a molten or aq form

40
Q

Metallic bonding

A

Giant lattice structure with a regular arrangement of positive metal ions held together in a sea of delocalised electrons.

41
Q

Uses of graphite? Why?

A

Electrodes bc it conducts electricity and has a high melting point.
Lubricant cuz its slippery

42
Q

Structure of graphite

A

Each carbon atom bonded to other 3 carbon atoms

Layers od hexagonal rings of carbon atoms

Weak intermolecular forces between layers

43
Q

Structure of silicon oxide

A

Each silicon atom is covalently bonded to 4 oxygen atoms

No delocalised electrons

Each oxygen atom is covalently bonded in 2 silicon atoms

44
Q

Why is diamond used in cutting tools

A

Its very hard

45
Q

Which properties do the structured silicon dioxide and diamond share

A

Very hard

Insoluble in water

Don’t conduct electricity

46
Q

Properties of graphite

A

High melting point
Slippery

47
Q

All carbon atom are covalently bonded to four other carbon atoms

A

No delocalised electrons

Chemistry (14 decks)

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