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Chemistry > Topic 3 Atoms, Element, Compounds > Flashcards

Topic 3 Atoms, Element, Compounds Flashcards

(68 cards)

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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
Proton numbers are also known as ________
Atomic numbers
26
Nucleon numbers are also known as _____
mass numbers
27
How to find nucleon number
nucelon = proton + neutrons
28
How are electrons arragned in an atom
arranged in shells around a nucleus
29
The arrangement of electron is also knwon as ________ __________
electronic configuration
30
Describe noble gases (2)
full outer electron shell stable ( doesn't react)
31
Define valence electrons
outer electrons of an element that are involved in chemical bonding
32
Why do element in the same group have similar chemical properties
same number of valence electrons
33
Define periodicity
A trend in a periodic table
34
Define isotope
Atoms of the same element with the same atomic number but different mass numbers
35
Why would isotopes of the same element have the same chemical properties?
same number of electrons in their electron shells
36
What is a chemical behaviour of an element determined by
outer electron shell
37
Define ion
when an atom loses or gains electrons in order to gain a full outer electron shell, gaining a charge
38
Define cations
positive charged ions
39
Define anions
negatively charged ions
40
How does ionic bonding happen?
forms due to METAL atoms giving their electrons to NON-METAL atoms in order for both atoms to become stable charged particles
41
Define ionic bond
electrostatic force of attraction between oppositely charged ions
42
Define ionic lattice
Ions in an ionic compound which are arranged in a pattern
43
Define oxidation
loss of electrons
44
Reduction
gain of electrons
45
Define electricity
flow of charged particles (ions or electrons)
46
Explain electrical conduction
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
Why can't conduction happen in ionic substances if solid
ions held in ionic lattice when solid, ions are not free to move about
48
How can conduction happen if an ionic substance is dissolved in a solution (or molten)
ionic lattice broken down, allowing the ions to more freely
49
Define electrolyte
Molten substance or a solution that conducts electricity
50
Non-metals (except graphite) and covalent substanes are electrical insulators True or False
True
51
Properties of ionic substances (5)
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
Define covalent bond
pair of electrons shared by two atoms, the shared part of the electrons holds the atoms together
53
define molecule
group of atoms held together by covalent bonds
54
Define valency
number of bonds an element needs to form in order gain a full outer electron shell
55
What is the valency for each group
1 2 3 4 3 2 1 0
56
What holds a covalent bond together
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
Define macromolecules
giant structures whose atoms are held together by multiple covalent bond
58
Define giant covalent structures
giant strucutres whose atoms are held together by multiple covalent bonds
59
Carbon has two forms which are classed as giant covalent structures. Name the two (2)
diamond graphite
60
Explain shape of diamond (2)
carbon atoms arranged in a tetrahedral structure every carbon is bonded to 4 other carbon atoms by very strong covalent bonds
61
explain shape of graphite (3)
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
Properties of diamonds (3)
all covalent bonding is strong high melting point as a lot of energy needed to break this strong bonds cannot conduct electricity
63
Properties of graphite (3)
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
Properties and explain silicon(IV) oxide (2)
forms 4 strong covalent bonds high melting point
65
Define covalent molecular substances
groups of atoms held together in molecules
66
Properties of covalent molecular substances (4)
low melting and boiling points volatile (vapourise easily) due to low melting and boiling points Does not conduct electricity insoluble in water
67
Explain why covalent molecular substances have low melting and boiling points (3)
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
Explain why giant covalent structures have high melting points
every strong covalent bonds must be broken, requring a lot of energy

Chemistry (11 decks)

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