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Chemistry > Topic 3 Atoms, Element, Compounds > Flashcards

Topic 3 Atoms, Element, Compounds Flashcards

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1
Q

Signs of chemical change (4)

A

temperature change

gas produced

changes in colour

percipitation/solid formed

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2
Q

Define physical reactions

A

reaction that involves change of state but no new substance is made

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3
Q

Physical substances are often easy to go back to the original substance.

True or false

A

true

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4
Q

What are reversible reactions indicated by?

A

⇌

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5
Q

Word equation for hydrated copper(II) sulfate

A

hydrated copper(II) sulfate ⇌ anyhdrous copper(II) sulfate + water

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6
Q

Word equation for hydrated cobalt (II) chloride

A

hydrated cobalt (II) chloride ⇌ anhydrous cobalt(II) chloride + water

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7
Q

Describe the colour change in hydrated copper(II) sulfate when it is heated and then water added again.

A

Hydrated copper(II) sulfate is BLUE

When heated, anhydrous copper(II) chloride formed. Colour is WHITE

If water is added, hydrated copper(II) sulfate formed again. Colour is blue.

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8
Q

Describe the colour change in hydrated cobalt(II) chloride when it is heated and then water added again.

A

hydrated cobalt(II) chloride is PINK

when heated, it forms anhydroous cobalt(II) chloride formed. Colour is BLUE

Adding water reconstructs hydrated cobalt(II) chloride. Colour is PINK

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9
Q

Define an element

A

substance containing only one type of atom

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10
Q

Define compound

A

substance containing two or more types of atoms chemically joined toether

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11
Q

Define mixture

A

Contains more than one substance but the substances are not chemically joined together

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12
Q

Features of metals (6)

A

conducts heat and electricity

malleable (easily bent or shaped)

shiny

sonorous (rings when struck)

ductile (stretches into a wire)

high melting and boiling point

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13
Q

Features of non-metals (4)

A

poor conductor of electricity

brittle

dull

low melting and boiling points

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14
Q

What are alloys

A

Formed when emtals are mixed with other elements

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15
Q

Define a solution

A

type of miture that is formed when one substance dissolves fully in another

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16
Q

define solute

A

substance that is dissolved

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17
Q

define solvent

A

substance which does the dissolving

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18
Q

Define concetration + units (2)

A

measure of how much solute is dissolved in the solvent

mol dm^-3 or moles per dm^3

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19
Q

Name the 3 sub-atomic particles

A

Proton

neutron

electron

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20
Q

Describe proton (3)

A

positive charge

Found within the nucleus of the atom

mass of 1

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21
Q

Describe neutron (3)

A

no charge

found within the nucleus of the atom

mass of 1

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22
Q

Describe electrons (3)

A

negative charge

found in the electron shells which orbit the nucleus

mass of about 1/2000

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23
Q

What is the overall charge of an atom

A

no over charge (number of protons = number of electrons)

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24
Q

The number of protons = number of electrons

True or false

A

True

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25
Q

Proton numbers are also known as ________

A

Atomic numbers

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26
Q

Nucleon numbers are also known as _____

A

mass numbers

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27
Q

How to find nucleon number

A

nucelon = proton + neutrons

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28
Q

How are electrons arragned in an atom

A

arranged in shells around a nucleus

29
Q

The arrangement of electron is also knwon as ________ __________

A

electronic configuration

30
Q

Describe noble gases (2)

A

full outer electron shell

stable ( doesn’t react)

31
Q

Define valence electrons

A

outer electrons of an element that are involved in chemical bonding

32
Q

Why do element in the same group have similar chemical properties

A

same number of valence electrons

33
Q

Define periodicity

A

A trend in a periodic table

34
Q

Define isotope

A

Atoms of the same element with the same atomic number but different mass numbers

35
Q

Why would isotopes of the same element have the same chemical properties?

A

same number of electrons in their electron shells

36
Q

What is a chemical behaviour of an element determined by

A

outer electron shell

37
Q

Define ion

A

when an atom loses or gains electrons in order to gain a full outer electron shell, gaining a charge

38
Q

Define cations

A

positive charged ions

39
Q

Define anions

A

negatively charged ions

40
Q

How does ionic bonding happen?

A

forms due to METAL atoms giving their electrons to NON-METAL atoms in order for both atoms to become stable charged particles

41
Q

Define ionic bond

A

electrostatic force of attraction between oppositely charged ions

42
Q

Define ionic lattice

A

Ions in an ionic compound which are arranged in a pattern

43
Q

Define oxidation

A

loss of electrons

44
Q

Reduction

A

gain of electrons

45
Q

Define electricity

A

flow of charged particles (ions or electrons)

46
Q

Explain electrical conduction

A

In metals (+ graphite) it is the outer electrons of the atoms (delocalised electrons) which are able to move and so can carry an electrric current

47
Q

Why can’t conduction happen in ionic substances if solid

A

ions held in ionic lattice when solid, ions are not free to move about

48
Q

How can conduction happen if an ionic substance is dissolved in a solution (or molten)

A

ionic lattice broken down, allowing the ions to more freely

49
Q

Define electrolyte

A

Molten substance or a solution that conducts electricity

50
Q

Non-metals (except graphite) and covalent substanes are electrical insulators

True or False

A

True

51
Q

Properties of ionic substances (5)

A

hard crystals- Due to strong attraction between positive and negatiev ions ionic substances are crystlline

high melting point- a lot of energy is needed to break the strong forces of attraction between ions

dissolves in water- water can form strong electrostatic attractions with the ions so are plucked off the lattice structure

does not conduct when solid- ions are held tightly in the lattice structure and are not able to move

conducts when molten/in solution- lattice breaks and ionsa re free to move

52
Q

Define covalent bond

A

pair of electrons shared by two atoms, the shared part of the electrons holds the atoms together

53
Q

define molecule

A

group of atoms held together by covalent bonds

54
Q

Define valency

A

number of bonds an element needs to form in order gain a full outer electron shell

55
Q

What is the valency for each group

A

1 2 3 4 3 2 1 0

56
Q

What holds a covalent bond together

A

protons (positive charged) held within nucleus

electrons (negative charged) held in electron shells outside nucleus

electron and proton attract as opposite charges attract, holding atom together in covalent bond

57
Q

Define macromolecules

A

giant structures whose atoms are held together by multiple covalent bond

58
Q

Define giant covalent structures

A

giant strucutres whose atoms are held together by multiple covalent bonds

59
Q

Carbon has two forms which are classed as giant covalent structures. Name the two (2)

A

diamond

graphite

60
Q

Explain shape of diamond (2)

A

carbon atoms arranged in a tetrahedral structure

every carbon is bonded to 4 other carbon atoms by very strong covalent bonds

61
Q

explain shape of graphite (3)

A

carbon atoms held in hexagonal shape, in layers

each carbon atoms bonds to three other cabons by strong covalent bonds

weak layers are held together by weak intermolecular forces of attractions

62
Q

Properties of diamonds (3)

A

all covalent bonding is strong

high melting point as a lot of energy needed to break this strong bonds

cannot conduct electricity

63
Q

Properties of graphite (3)

A

strong covalent bonds between atoms but weak intermolecular forces of attraction between layers

layer can slide over one another, LUBRICANT (substance that minimizes friction)

Conducts electricity because graphtie contains delocalised electron

64
Q

Properties and explain silicon(IV) oxide (2)

A

forms 4 strong covalent bonds

high melting point

65
Q

Define covalent molecular substances

A

groups of atoms held together in molecules

66
Q

Properties of covalent molecular substances (4)

A

low melting and boiling points

volatile (vapourise easily) due to low melting and boiling points

Does not conduct electricity

insoluble in water

67
Q

Explain why covalent molecular substances have low melting and boiling points (3)

A

when melted or boiled, the strong bonds between atoms (intramolecular forces) are not broken

Instead the intermolecular forces (weak forces of attraction been molecules) are broken

Intermolecular forces of attraction much weaker than intramolecular forces of attraction

68
Q

Explain why giant covalent structures have high melting points

A

every strong covalent bonds must be broken, requring a lot of energy

Chemistry (11 decks)

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