Untitled Deck Flashcards
1
Q
What is matter made of?
A
Matter is made of atoms
Matter includes solids, liquids, and gases.
2
Q
What charge do atoms have?
A
Atoms have a neutral charge
This means they contain equal numbers of positive and negative charges.
3
Q
What happens when a rod is rubbed with a cloth?
A
Electrons are rubbed off one object and onto the other, causing the objects to become charged.
4
Q
What charge does the cloth have after rubbing?
A
The cloth has a positive charge
It has more positives after losing electrons.
5
Q
What charge does the rod have after rubbing?
A
The rod has a negative charge
It has more negatives after gaining electrons.
6
Q
What forces do charged objects exert on each other?
A
Attraction or repulsion
7
Q
What does the term ‘atom’ mean?
A
‘Atom’ comes from the Greek word meaning ‘indivisible’.
8
Q
Who thought the smallest unit of matter could not be cut up further?
A
The Greek philosopher Democritus.
9
Q
What three sub-atomic particles make up an atom?
A
- Protons (+)
- Electrons (-)
- Neutrons (neutral)
10
Q
Where are electrons located in an atom?
A
Electrons orbit the nucleus in shells.
11
Q
What is the atomic number?
A
Atomic number = protons in nucleus.
12
Q
What determines the kind of atom it is?
A
The number of protons in an atom.
13
Q
What is an element?
A
A pure substance where all atoms have the same atomic number.
14
Q
What is the mass number?
A
Mass number = protons + neutrons together.
15
Q
What are isotopes?
A
Atoms with the same number of protons but different numbers of neutrons.
16
Q
How do you calculate the number of neutrons?
A
Neutrons = mass number - atomic number.
17
Q
What happens to the mass number when neutrons change?
A
The mass number changes, leading to different isotopes.
18
Q
What is the mass of an electron compared to a proton?
A
The mass of an electron is 1/1840th of the mass of a proton.
19
Q
How many electrons can the first shell hold?
A
The first shell can hold up to 2 electrons.
20
Q
What happens to the outer shell electrons as you move down a group in the periodic table?
A
The number of outer shell electrons remains the same.
21
Q
What characterizes Group 1 Alkali Metals?
A
- Highly reactive
- Soft and can be cut with a knife
- Float and fizz in water
22
Q
What characterizes Group 2 Alkali Earth Metals?
A
- Less reactive than Group 1
- Grey-white and shiny
- Good conductors of electricity
23
Q
What characterizes Group 17 Halogens?
A
- Non-metals
- Toxic and reactive
- Reactivity decreases down the group
24
Q
What characterizes Group 18 Noble Gases?
A
- Non-metals
- Colourless gases
- Completely unreactive
25
What is the significance of the periodic table rows?
The rows correspond to the number of electron shells.
26
What is the significance of the periodic table groups?
The group has similar elements according to their properties.
27
What is the electron configuration of an atom?
The distribution of electrons in an atom's electron shells.
28
What are the two forms of the same element called?
Isotopes.
29
Name two ways that the isotopes of chlorine are the same.
* Same atomic number
* Same chemical properties
30
Give one way in which the isotopes of chlorine are different.
Different mass numbers.
31
Which elements are of the same element from the group of four: Q, X, Y, Z?
Elements X and Y (if they are the same element).
32
What do alkali metals, halogens, and noble gases have in common?
They are all groups in the Periodic Table.
33
What is the formula for a chemical reaction?
Reactant + Reactant → Product.
34
What happens to atoms during a chemical reaction?
They form new substances with different chemical properties.
35
What are ions?
Charged atoms formed when atoms gain or lose electrons.
36
What is an ionic bond?
The force of attraction between oppositely charged ions.
37
What types of elements typically form ionic bonds?
Metals and non-metals.
38
What is the crystal lattice structure in ionic compounds?
A structure where positive and negative ions attract each other.
39
What must all chemical substances be?
Electrically neutral.
40
What does the formula for a substance made of ions represent?
The simplest ratio of different ions.
41
What does the term 'cation' refer to?
A positively charged ion.
42
What does the term 'anion' refer to?
A negatively charged ion.
43
How does a molecule form?
When two or more non-metal atoms join together through covalent bonding.
44
What is a covalent bond?
A bond formed when atoms share electrons.
45
Name a common example of a covalent molecule.
H2O (water).
46
What is the difference between CO2 and CO?
CO2 is carbon dioxide; CO is carbon monoxide.
47
What is the maximum number of electrons the first shell can hold?
2 electrons.
48
What is the atomic number?
The number of protons in an atom.
49
What is the mass number?
The total number of protons and neutrons in an atom.
50
True or False: All atoms are electrically neutral.
True.
51
What is a common property of noble gases?
They are inert and do not easily form compounds.
52
What happens to metals during ionic bonding?
They lose electrons to become positively charged.
53
What happens to non-metals during ionic bonding?
They gain electrons to become negatively charged.
54
What is the formula for magnesium oxide?
MgO.
55
What is the formula for calcium chloride?
CaCl2.
56
Fill in the blank: Ionic bonding occurs between _______ and non-metals.
metals.
57
What is the charge on a sodium ion?
+1.
58
What is the charge on a sulfate ion?
-2.
59
What is the formula for sodium sulfate?
Na2SO4.
60
What is the formula for ammonium nitrate?
NH4NO3.
61
What do covalent bonds form between?
Two or more non-metals.
62
True or False: Covalent bonds are weaker than ionic bonds.
False.
63
What is one example of a diatomic molecule?
O2 (oxygen).
64
What is the significance of the formula of a covalent molecule?
It shows how many atoms of each element are present.
65
What is the formula for ozone?
O3.
66
What does the term 'electrostatic attraction' refer to?
The attraction between positively and negatively charged particles.
67
What is the role of shared electrons in a covalent bond?
They create a bond by being attracted to both nuclei.
68
How can you identify non-metals in ionic compounds?
They typically have negative charges.
69
What do molecules made of covalent bonds consist of?
Groups of atoms chemically bonded together.
70
What is the charge of a fluoride ion?
-1.
71
What is the charge of a phosphate ion?
-3.
72
The second energy level in its valence (outer) shell is __.
8
73
Chlorine 17Cl has an electron structure that can be written as Cl: __.
2, 8, 7
74
What is the electron structure of a sodium atom?
2, 8, 1
75
What is the electron structure of a sodium ion Na+?
2, 8
76
Why is the sodium ion less reactive than the sodium atom?
It has a full outer shell
77
Why would the sodium ion be smaller than the sodium atom?
It has lost an electron
78
Why is the sodium ion not Na2+?
It has only lost one electron
79
What is the electron structure of Cl and Cl-?
Cl: 2, 8, 7 / Cl-: 2, 8, 8
80
Why is the charge on the chloride ion?
-1
81
Why is the chloride ion less reactive than the chlorine atom?
It has a full outer shell
82
Why is the chloride ion Cl- not Cl2-?
Cl only gains one electron
83
State the chemical formula for magnesium chloride.
MgCl2
84
State the chemical formula for magnesium carbonate.
MgCO3
85
State the chemical formula for ammonium carbonate.
(NH4)2CO3
86
State the chemical formula for calcium carbonate.
CaCO3
87
State the chemical formula for silver nitrate.
AgNO3
88
State the chemical formula for copper sulfate.
CuSO4
89
State the chemical formula for ammonium hydroxide.
NH4OH
90
State the chemical formula for zinc oxide.
ZnO
91
State the chemical formula for sulfuric acid.
H2SO4
92
State the chemical formula for iron (II) sulfate.
FeSO4
93
State the chemical formula for iron (II) chloride.
FeCl2
94
State the chemical formula for potassium chloride.
KCl
95
State the chemical formula for copper chloride.
CuCl2
96
State the chemical formula for sodium fluoride.
NaF
97
State the chemical formula for ammonium nitrate.
NH4NO3
98
State the chemical formula for iron (II) sulfide.
FeS
99
State the chemical formula for aluminium chloride.
AlCl3
100
State the chemical formula for calcium hydroxide.
Ca(OH)2
101
What is the name of the compound FeS?
Iron (II) sulfide
102
What is the name of the compound ZnO?
Zinc oxide
103
What is the name of the compound Al2O3?
Aluminium oxide
104
What is the name of the compound CuSO4?
Copper(II) sulfate
105
What is the name of the compound Na2S?
Sodium sulfide
106
What is the name of the compound NaOH?
Sodium hydroxide
107
What is the name of the compound Pb(NO3)2?
Lead(II) nitrate
108
What is the name of the compound Ca3(PO4)2?
Calcium phosphate
109
What is the name of the compound Fe2O3?
Iron(III) oxide
110
What is the name of the compound NaNO3?
Sodium nitrate
111
What is the name of the compound AgCl?
Silver chloride
112
What is the name of the compound CuCO3?
Copper(II) carbonate
113
What is the name of the compound Ca(OH)2?
Calcium hydroxide
114
What is the name of the compound Al2(SO3)3?
Aluminium sulfite
115
Elements on the left side of the Periodic Table tend to _______.
lose electrons
116
Elements on the right side of the Periodic Table tend to _______.
gain electrons
117
Which elements are considered metals?
Sodium, magnesium, aluminium
118
Which groups include non-metals?
15, 16, 17, 18
119
What is the rule for balancing equations?
Change coefficients only, not subscripts
120
What is the first step in balancing an equation?
Check the formulas for the products
121
What must be written with a subscript of 2 when they appear alone?
Diatomic molecules
122
What are the steps to balance an equation?
Balance metals, non-metals, oxygen, hydrogen
123
What is the atomic number?
Number of protons
124
What is the mass number?
Protons + Neutrons
125
Define isotope.
Atoms of the same element with different numbers of neutrons
126
What is an example of an isotope?
Carbon-14
127
Group 1 elements are known as _______.
Alkali metals
128
Group 2 elements are known as _______.
Alkaline earth metals
129
Group 16 elements are known as _______.
Chalcogens
130
Group 17 elements are known as _______.
Halogens
131
Group 18 elements are known as _______.
Noble gases
132
What is a covalent bond?
A bond formed by sharing electrons
133
What is an ionic bond?
A bond formed by the transfer of electrons
134
How do ions become positively or negatively charged?
By losing or gaining electrons
135
What is the Swap, Drop and Cancel rule used for?
Writing formulas for ionic compounds
136
What is the significance of compounds being electrically neutral?
Positive and negative charges balance out
137
Draw and label an atom.
Nucleus, protons, neutrons, electrons
