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Chemistry Flashcards

1
Q

STRUCTURE AND BONDING

A
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2
Q
  1. What can link two atoms together?
A

a bond

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3
Q
  1. Which group of elements is stable and doesnt form compounds easily?
A

noble gases/group 0 in the periodic table

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4
Q
  1. How is an elements electron arrangement linked to its position in the periodic table?
A

Elements in the same group have the same number of electrons in their outer shell.

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5
Q
  1. How do positive and negative charges affect each other?
A

They attract each other.

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6
Q
  1. Which sub-atomic particles of atoms take part in chemical reactions?
A

electrons

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7
Q
  1. What is an ion?
A

an atom that is charged because it has lost or gained one or more electrons

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8
Q
  1. What happens when an ionic bond is formed?
A

One atom loses electrons to another atom to form oppositely charged ions that attract each other.

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9
Q
  1. Which kinds of elements are usually involved in the formation of ionic bonds?
A

metals and non-metals

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10
Q
  1. How is a positive ion formed and what is it called?
A

formed by the loss of electrons; cation

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11
Q
  1. How is a negative ion formed and what is it called?
A

formed by the gain of electrons; anion

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12
Q
  1. What are the forces called that hold ions together?
A

electrostatic forces / electrostatic attractions / ionic bond

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13
Q
  1. Why do atoms form ions?
A

to become more stable (like a noble gas)

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14
Q
  1. Explain why group 1 elements such as sodium and lithium form a 1+ ion.
A

They both have one electron in their outer shell and lose it to become stable.

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15
Q
  1. What are the charges on calcium, oxide and chloride ions?
A

2+, 2- and 1-

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16
Q
  1. What structure of regularly repeating ions do ionic compounds form?
A

lattice structure / ionic lattice

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17
Q
  1. What is the formula of the nitrate ion?
A

NO3

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18
Q
  1. What is the general name for a positive ion?
A

cation

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19
Q
  1. What is the general name for a negative ion?
A

anion

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20
Q
  1. What is the charge on the ions of elements in group 1 of the periodic table?
A

+1

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21
Q
  1. What is the charge on the ions of elements in group 6 of the periodic table?
A

-2

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22
Q
  1. What happens to the electrons in the outer shell of metal atoms when they form ions?
A

they are lost

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23
Q
  1. What is the name of the ionic compound containing calcium and bromine only?
A

calcium bromide

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24
Q
  1. What is the name of the ionic compound containing potassium, chlorine and oxygen?
A

potassium chlorate (any element combined with oxygen is an ___ate )

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25
Q
  1. What does a bond do in an element or compound?
A

holds atoms together

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26
Q
  1. What are electrostatic forces of attraction?
A
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27
Q
  1. Which part of an atoms structure is most involved when two atoms react?
A
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28
Q
  1. How many electrons are in the outer shell of the elements in groups 5, 6 and 7?
A
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29
Q
  1. What kind of electron arrangement is most stable?
A
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30
Q
  1. What is the molecular formula of the very common compound formed between hydrogen and oxygen?
A
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31
Q
  1. How many more electrons does an oxygen atom need to get a complete outer shell?
A
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32
Q
  1. What are molecules?
A
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33
Q
  1. Which type of atoms are covalent bonds found between
A
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34
Q
  1. What is a covalent bond?
A
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35
Q
  1. What happens to electrons between two atoms in a covalent bond
A
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36
Q
  1. What kinds of elements usually form molecules?
A
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37
Q
  1. What kinds of bonds are found in molecules?
A
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38
Q
  1. What is the name of the type of bond formed by sharing electron pairs within molecules?
A
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39
Q
  1. What term describes the number of atoms of each element bonded together in a molecule?
A
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40
Q
  1. In oxygen and carbon dioxide, the atoms share two pairs of electrons. How do we describe these bonds?
A
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41
Q
  1. What is the name of the force that holds molecules together in gases and liquids
A
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42
Q
  1. How strong are the forces of attraction between molecules compared to the bonds within molecules?
A
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43
Q
  1. Are simple molecules usually good conductors of electricity at room temperature?
A
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44
Q
  1. In what types of bonds are pairs of electrons shared?
A
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45
Q
  1. What are intermolecular forces?
A
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46
Q
  1. Do simple molecules have strong intermolecular forces between them?
A
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47
Q
  1. Why are simple molecules poor conductors of electricity?
A
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48
Q
  1. What can you say about the formula of small, simple molecules?
A
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49
Q
  1. What type of bonding is between the atoms in a molecule of water?
A
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50
Q
  1. What type of structure does water have?
A
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51
Q
  1. What strength of forces are there between different molecules of water?
A
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52
Q
  1. Does pure water conduct electricity?
A
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53
Q
  1. What type of structure do diamond and graphite have?
A
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54
Q
  1. What does the term malleable mean?
A
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55
Q
  1. What type of bonding does copper have?
A
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56
Q
  1. What atoms does metallic bonding happen between?
A
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57
Q
  1. What holds ions of metals together in a metallic bond?
A
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58
Q
  1. Why can metals conduct electricity?
A
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59
Q
  1. What is a metallic bond?
A
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60
Q
  1. What are the particles inside a metal?
A
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61
Q
  1. Metals are ductile. What does ductile mean?
A
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62
Q

ACIDS AND ALKALIS

A
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63
Q
  1. What term describes a substance that attacks metals, stonework and skin?
A

corrosive

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64
Q
  1. Name an acidic solution found in the kitchen.
A

vinegar or fruit juice, etc.

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65
Q
  1. Name an alkaline solution used in the kitchen.
A

bleach or oven cleaner or soap, etc.

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66
Q
  1. What type of substance turns litmus paper red?
A

acid

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67
Q
  1. How does an indicator show the acidity or alkalinity of solutions?
A

by changing colour`

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68
Q
  1. What pH values represent alkaline solutions?
A

above 7 or 8 to 14

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69
Q
  1. What happens in all chemical reactions?
A

new substances are formed

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70
Q
  1. What kind of reaction occurs between an acid and an alkali?
A
  1. What kind of reaction occurs between an acid and an alkali?
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71
Q
  1. What do you call a solution that is neither acidic nor alkaline.
A
  1. What do you call a solution that is neither acidic nor alkaline.
72
Q
  1. Give the name and formula of a common laboratory acid.
A

hydrochloric acid (HCl) or nitric acid (HNO3) or sulfuric acid (H2SO4), etc.

73
Q
  1. Which ion is in excess in all acidic solutions?
A

hydrogen ions or H+ ions

74
Q
  1. Which ion is in excess in all alkaline solutions?
A

hydroxide ions or OH– ions

75
Q
  1. What scale is used for measuring acidic and alkaline properties?
A

the pH scale

76
Q
  1. Name three examples of acid/alkali indicators apart from universal indicator.
A

litmus, methyl orange and phenolphthalein

77
Q
  1. What would you use to measure pH to one decimal place?
A

a pH meter

78
Q
  1. What pH values are acidic?
79
Q
  1. What colour is phenolphthalein in a solution with a pH of 2?
A

colourless

80
Q
  1. What happens to the pH as the H+ ion concentration increases?
A

it decreases

81
Q
  1. If a solution has the same concentration of hydrogen ions as hydroxide ions, how is it described?
A

neutral or pH = 7

82
Q
  1. If 2 g of salt is dissolved in 250 cm3 of solution, what is its concentration in g dm–3?
A

8 g dm–3

83
Q
  1. What word describes a solution that contains a large amount of solute in a small volume of solvent?
A

concentrated

84
Q
  1. How can a solution be made more dilute?
A

by adding solvent/water

85
Q
  1. If 24 g of acid is dissolved in 600 cm3 of solution, what is its concentration in g dm–3?
A

40 g dm–3

86
Q
  1. What happens when strong acid molecules dissolve in water?
A

they dissociate completely into ions

87
Q
  1. What kind of reaction occurs between an acid and a base?
A

neutralisation

88
Q
  1. What happens to the pH of an acid as it reacts with a neutraliser?
A

pH increases

89
Q
  1. What is formed when an acid reacts with a base like a metal oxide?
A

salt + water

90
Q
  1. What acid would be used to make zinc sulfate from zinc oxide?
A

sulfuric acid (sulphuric acid makes sulphates!)

91
Q
  1. What process can be used to separate an insoluble solid from a liquid?
92
Q
  1. How can a sample of a dissolved salt be obtained from a salt solution?
93
Q
  1. In general, what is the pH of an alkaline solution?
94
Q
  1. In general, what is the pH of an alkaline solution?
95
Q
  1. What colour is litmus solution in acidic solutions?
96
Q
  1. What name is given to substances that react with acids to form a salt and water only?
97
Q
  1. Which salt is formed when copper oxide reacts with sulfuric acid?
98
Q
  1. What type of reaction happens between an acid and a base?
99
Q
  1. What type of solution has a pH of 7?
100
Q
  1. Name the acid that has the formula HCl.
101
Q
  1. What colour is phenolphthalein in alkaline solutions?
102
Q
  1. What is the formula for sulfuric acid?
103
Q
  1. Name the salt produced when sodium hydroxide reacts with hydrochloric acid.
104
Q
  1. Which ions, hydrogen ions or hydroxide ions, are released by acids in solution?
105
Q
  1. What substance, other than a salt, is produced when an alkali neutralises an acid?
106
Q
  1. What name is given to substances that are soluble bases?
107
Q
  1. What is the formula for hydrochloric acid?
108
Q
  1. What type of solution has a pH above 7?
109
Q
  1. What colour is phenolphthalein in acidic solutions?
110
Q
  1. Name a piece of apparatus used to measure volumes of liquid.
111
Q
  1. Name the separation method used to produce crystals from a solution.
112
Q
  1. Name the acid needed to make ammonium nitrate.
113
Q
  1. Which acid can be used to make copper sulfate?
114
Q
  1. Which base can be used to make copper sulfate?
115
Q
  1. Which substance is needed to complete the general equation: acid + base makes salt + …?
116
Q
  1. What is the formula of nitric acid?
117
Q
  1. What is the name of the salt formed from zinc oxide and hydrochloric acid?
118
Q
  1. What is the formula of the salt formed from calcium oxide and hydrochloric acid?
119
Q
  1. Which ions are present in large quantities in aqueous solutions of all acids?
120
Q
  1. Which ions are present in large quantities in aqueous solutions of all alkalis?
121
Q
  1. Which gas is formed when dilute hydrochloric acid reacts with magnesium?
122
Q
  1. Which gas is formed when dilute hydrochloric acid reacts with magnesium carbonate?
123
Q
  1. What acid can be used to make copper chloride?
124
Q
  1. What gas is given off when magnesium reacts with dilute sulfuric acid?
125
Q
  1. How do you identify Hydrogen gas?
126
Q
  1. What is seen when magnesium is added to dilute sulfuric acid?
127
Q
  1. What is the formula of magnesium sulfate?
128
Q
  1. What gas is produced when copper carbonate is added to dilute nitric acid?
129
Q
  1. How do you test for Carbon Dioxide?
130
Q
  1. What is the formula of the salt produced when copper carbonate reacts with nitric acid?
131
Q
  1. Sodium chloride dissolves in water to form a solution. Which is the solute?
132
Q
  1. What do we call the liquid that dissolves a solute to form a solution.
133
Q

MASS CALCULATIONS, ELECTROLYSIS, EXTRACTION OF METALS AND EQUILIBRIA

134
Q
  1. The formula of magnesium chloride is MgCl2. What is the ratio of magnesium ions to chloride ions?
135
Q
  1. The formula of sulfuric acid is H2SO4. How many atoms of each element are in the formula?
A

H = 2, S = 1, O = 4

136
Q
  1. The formula of calcium nitrate is Ca(NO3)2. How many calcium, nitrogen and oxygen atoms are in the formula?
A

Ca = 1, N = 2, O = 6

137
Q
  1. There are two numbers alongside chlorine in the periodic table, 17 and 35.5. What does the number 17 represent?
A

atomic number

138
Q
  1. What does the number 35.5 represent?
A

relative atomic mass

139
Q
  1. Sodium chloride has the formula NaCl. The relative atomic mass of sodium is 23 and that of chlorine is 35.5. What is the relative formula mass of NaCl?
140
Q
  1. A water molecule has the formula H2O. The relative atomic mass of hydrogen is 1 and that of oxygen is 16. What is the relative formula mass of a molecule of water?
141
Q
  1. What is the symbol for relative atomic mass?
142
Q
  1. What is the symbol for relative formula mass?
143
Q
  1. The relative atomic mass of hydrogen is 1. What is the relative formula mass of hydrogen molecules?
144
Q

IVE GIVEN UP WITH THE NUMBERS IF THEY SEEM FUCKY THEY PROBABLY ARE <3

145
Q
  1. A carbon dioxide molecule has the formula CO2; the relative atomic mass of carbon is 12 and that of oxygen is 16. What is the relative formula mass of carbon dioxide?
146
Q
  1. What is the empirical formula of a compound with molecular formula C2H4?
147
Q
  1. What is the empirical formula of a compound with molecular formula C3H8?
148
Q
  1. A sample of magnesium carbonate was heated in an open test tube. Why did it lose mass?
A

gas/carbon dioxide escaped

149
Q

100 cm3 of a solution contained 2 g of salt. What is the concentration of the salt in g dm-3?

150
Q
  1. A sample of copper carbonate was heated in an open test tube. Why did it lose mass?
A

gas/carbon dioxide escaped

151
Q
  1. Why does magnesium increase in mass when it is heated in air?
A

combines with oxygen

152
Q
  1. How many cm3 are there in 1 dm3?
153
Q
  1. What is 250 cm3 expressed in dm3?
154
Q
  1. What is 0.5 dm3 expressed in cm3?
155
Q

100 cm3 of a solution contains 1.5 g of salt. What is the concentration of the salt solution in g dm3?

156
Q

250 cm3 of a solution contains 5 g of sugar. What is the concentration of the sugar solution in g dm3?

157
Q
  1. A solution of copper sulfate has concentration 10 g dm3. What mass of copper sulfate will be dissolved in 100 cm3 of solution?
158
Q

2 g of hydrogen reacts with oxygen to form 18 g of water. What mass of water will be formed from 1 g of hydrogen?

159
Q

2H2 + O2 → 2H2O. How many molecules of hydrogen are needed to react with 1 dozen molecules of oxygen to form water?

160
Q
  1. What is the abbreviation used for the mole, the unit for amount of substance?
161
Q
  1. How many particles are there in 1 mole of particles?
A

6.02 x 1023 (Avrogadros number)

162
Q
  1. The mass of 1 mole of carbon atoms is 12 g. What is the mass of 2 moles of carbon atoms?
163
Q
  1. What is the formula for calculating the number of moles of substance from its mass in g
A

moles = mass (g) / RAM or RFM

164
Q
  1. Each water molecule contains three atoms. How many moles of atoms are there in 2 moles of water molecules?
165
Q
  1. The relative formula mass of chlorine gas is 71. What is the mass of 1 mole of chlorine gas?
166
Q
  1. What is the Avogadro number?
A

the number of atoms/particles in a mole

167
Q
  1. What is the emperical formula of a compound?
A

The simplest whole number ratio of atoms in compound

168
Q
  1. What is the law of conservation of mass?
A

total mass of reactants = total mass of products

169
Q
  1. How are the emperical formula and molecular formula related?
A

The molecular formula is a multiple of the emperical formula

170
Q
  1. What name is given to an atom that has gained or lost electrons?
171
Q
  1. What type of charge is on metal and hydrogen ions?
172
Q
  1. What type of charge is on most non-metal ions?
A
  1. What type of charge is on most non-metal ions?
173
Q
  1. What is another name for a positive ion?
174
Q
  1. What is another name for a negative ion?
175
Q

listen. I appreciate you guys and all but ive been doing this for too long. I’ve put the link to the other brainscape thing so you can read the questions. you have to click on the “preview the cards in this deck” button (the glasses). currently, we’re in “Topic 5a Mass calculations, electrolysis, extraction of metals and equilibria Flashcards Preview” at question 44. im tired and im going to bed. also gonna fail chemistry but shhh its not important-

A

https://www.brainscape.com/l/dashboard/edexcel-gcse-chemistry-2022-17311240/decks

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