EDEXCEL GCSE 9-1 COMBINED SCIENCE FOUNDATION CHEMISTRY PAPER 1+2

?
  • Created by: jordanb-h
  • Created on: 15-03-18 21:36
what is an element?
is a substance made from atoms with the same number of protons in the nucleus. Each element has its own chemical symbol, which: consists of one or two letters, starts with a chemical letter and has any other letters in lower case
1 of 140
What is meant by the term ion?
An ion is a charged particle formed when an atom, or group of atoms, loses or gains electrons
2 of 140
what is a compound?
a compound consists of two or more different elements chemically joined together
3 of 140
what is an atom?
is the smallest particle of an element that still has its chemical properties
4 of 140
what is a molecule?
A molecule consists of two or more atoms chemically joined together
5 of 140
in a chemical reaction what are the reactants?
are the substances that undergo a chemical change in a reaction
6 of 140
in a chemical reaction what are the products?
are the new substances formed
7 of 140
what do state symbols show ?
show the physical state of each substance in a balanced equation
8 of 140
What is the state symbol for Solid
(s)
9 of 140
What is the state symbol for liquid
(l)
10 of 140
what is the state symbol for gas
(g)
11 of 140
what is the state symbol for aqueous solution
(aq)
12 of 140
what is a hazard?
is something that could: cause damage or harm to someone or something, cause negative health effects which may occur immediately or later on
13 of 140
what is a risk?
is the chance that someone or something will be exposed to a hazard. The amount of risk depends on factors such as: how much someone is exposed to a hazard, the way in which exposure happens and how series the effects of exposure are
14 of 140
what are hazard symbols intended to do?
warn about the dangers of the substance in the container and let people know about the precautions to take when they use the substance
15 of 140
what is a precaution?
is something that you can do to reduce the risk of harm from a hazard
16 of 140
what do precautions include?
using smaller amounts of a hazardous substance, use protective clothing and using a different method or apparatus
17 of 140
In 1803 who described the structure of the atom as a solid atom model: all atoms of an element are identical; different elements have different atoms
Dalton
18 of 140
who discovers the electron in the atomic structure ?
Thomson , 1897
19 of 140
In 1911 Rutherford described the structure of an atom using what model?
solar system model: atoms have a positive nucleus surrounded by negative electrons in orbit
20 of 140
In 1913 Bohr described the structure of an atom using what model?
electron shell model: electrons occupy shells or energy levels around the nucleus
21 of 140
who discovers the proton in the atomic structure?
Rutherford, 1918
22 of 140
who discovers the neutron in the atomic structure?
Chadwick, 1932
23 of 140
what does an atom consist of?
a central nucleus, which: contains protons and neutrons, is surrounded by electrons in shells
24 of 140
each atom can be described by what?
its mass number, the total number of protons and neutrons in the nucleus
25 of 140
each atom can be described by what?
its atomic number, the number of protons in the nucleus
26 of 140
atoms of a given element have ?
the same number of protons in the nucleus: all have the same atomic number, this number is unique to that element
27 of 140
what are isotopes?
are atoms of an element with: the same number of protons and different numbers of neutrons
28 of 140
how do you calculate the number of neutrons?
mass number- atomic number
29 of 140
what do Ar values take into account?
the relative abundance or percentage of each isotope in a sample of an element. The existence of isotopes means that the Ar values of elements may not be whole numbers. Mass numbers can only be whole numbers.
30 of 140
In Ar values why can only mass numbers be whole numbers?
this is because you can't have parts of protons or neutrons in an atom
31 of 140
What is the relative charge for a proton?
+ 1
32 of 140
What is the relative mass for a proton?
1
33 of 140
What is the relative charge for a neutron?
0
34 of 140
What is the relative mass for a neutron?
1
35 of 140
What is the relative charge for a electron?
-1
36 of 140
What is the relative mass for a electron?
1/1836
37 of 140
Atoms have equal numbers of what?
protons and electrons. They have equal numbers of positive and negative charges, and so are neutral overall
38 of 140
Electrons have very little what?
mass compared with protons and neutrons. Most of the mass of an atom is concentrated in its nucleus
39 of 140
who's periodic table was successful and developed into the modern periodic table
Dimitri Mendleev's
40 of 140
At first how did Mendeleev arrange the elements?
in order of relative atomic mass. However he reversed the position of some pairs of elements. This matched the properties of the elements and their compounds
41 of 140
Mendeleev left gaps in his table. Explain the importance of doing this
The gaps were for elements not discovered then. Mendeleev used his table to predict the properties of these elements. When they were discovered later, their properties closely matched his predicted properties.
42 of 140
what is the modern periodic table useful for?
describing and predicting properties of elements
43 of 140
In Mendeleev's periodic table, atomic number was what?
just the position of an element in the table
44 of 140
what did later discoveries show?
atomic number is actually the number of protons in the nucleus of an atom
45 of 140
what did later discoveries show?
each element has a unique atomic number
46 of 140
what did later discoveries show?
if the elements are arranged in order of increasing atomic number, Mendeleev's pair reversals are explained
47 of 140
in the periodic table what are the horizontal rows called
periods
48 of 140
in the periodic table metals are on the left-hand side and where
in the centre
49 of 140
in the periodic table elements with similar properties are placed in the same what
vertical groups
50 of 140
where are non-metals in the periodic table?
on the right-hand side
51 of 140
what describes the arrangement of electrons in an atom?
electronic configuration
52 of 140
In an atom electrons occupy what?
electron shells
53 of 140
In an atom shells are filled, starting with what?
the innermost shell
54 of 140
In an atom different shells hold what?
different maximum numbers of electrons
55 of 140
What is an ion?
is an atom or a group of atoms with a positive or negative charge
56 of 140
cations usually form from what?
hydrogen or metals: group 1 atoms lose 1 electron to form ions with one positive charge, Group 2 atoms lose 2 electrons to form ions with two positive charges
57 of 140
what is an anion?
a negatively charged ion formed when an atom or group of atoms gains one or more electrons
58 of 140
anions usually form from what?
non-metals: Group 7 atoms gain 1 electron to form ions with one negative charge, Group 6 atoms gain 2 electrons to form ions with two negative charges
59 of 140
what does an ion's name depend on?
the charge and whether the ion also contains oxygen. Compound ions contain atoms of two different elements
60 of 140
what is the formula for Hydrogen
H+
61 of 140
what is the formula for Lithium (group 1)
Li+
62 of 140
what is the formula for Sodium (group 1)
Na+
63 of 140
what is the formula for Potassium (group 1)
K+
64 of 140
what is the formula for Magnesium (group 2)
K+
65 of 140
what is the formula for Calcium (group 2)
Ca2+
66 of 140
what is the formula for Barium (group 2)
Ba2+
67 of 140
what is the formula for Aluminium (group 3)
Al3+
68 of 140
what is the formula for Silver (transition metal)
Ag+
69 of 140
what is the formula for Copper (transition metal)
Cu2+
70 of 140
what is the formula for Zinc (transition metal)
Zn2+
71 of 140
what is the formula for Iron II (transition metal)
Fe2+
72 of 140
what is the formula for Iron III (transition metal)
Fe3+
73 of 140
what is the formula for Ammonium (compound ion)
NH4+
74 of 140
Negatively charged ions formed from single non-metal atoms take the name of the element but end in what?
-ide
75 of 140
Negatively charged ions in compounds containing three or more elements, one of which is oxygen end in what?
-ate
76 of 140
what is the formula for Fluoride (group 7)
F-
77 of 140
what is the formula for Chloride (group 7)
Cl-
78 of 140
what is the formula for Bromide (group 7)
Br-
79 of 140
what is the formula for Iodide (group 7)
I-
80 of 140
what is the formula for Oxide (group 6)
O2-
81 of 140
what is the formula for Sulfide (group 6)
S2-
82 of 140
what is the formula for Nitrate (compound ion)
NO3-
83 of 140
what is the formula for Carbonate (compound ion)
CO3 2-
84 of 140
what is the formula for Sulfate (compound ion)
SO4 2-
85 of 140
what is the formula for Hydroxide (compound ion)
OH-
86 of 140
Ionic bonds are what?
strong electrostatic forces of attraction between oppositely charged ions
87 of 140
The ions in a ionic compound from a what ?
lattice structure which has: a regular arrangement of ions and ionic bonds are between oppositely charged ions
88 of 140
Ionic compounds usually have what?
high melting points and high boiling points
89 of 140
Ionic compounds are often what?
soluble in water. They dissolve to form aqueous solutions
90 of 140
An electric current is a flow of charge. A substance will conduct electricity if what?
it contains charge carriers (such as ions), these charge carriers are free to move through the substance
91 of 140
State why sodium chloride does not conduct electricity when it is in the solid state
The ions are not free to move around in a solid
92 of 140
Explain why sodium chloride does conduct electricity when it is molten or in aqueous solution
The ions are free to move around when sodium chloride is liquid or when it is dissolved in water. This means they can carry electric charge from place to place
93 of 140
Covalent bonds are what
are strong, form between non-metal atoms and often produce molecules, which can be elements or compounds
94 of 140
What does a Simple Molecular consist of?
just a few atoms, joined to each other by strong covalent bonds.
95 of 140
What can Simple Molecular substances be?
non-metal elements and compounds of non-metals
96 of 140
What do Simple Molecular substances usually have?
low melting points, low boiling points
97 of 140
What state are simple molecular substances are at room temperature?
gas or liquid state
98 of 140
Simple Molecular Substances do not conduct electricity when they are solid, liquid or gas. Why is this?
This is because their molecules: are not electrically charged and do not contain electrons that are free to move
99 of 140
Most simple molecular substances do not conduct electricity when in a solution. However ?
some of them such as acids break down when they dissolve form ions and these ions can move around so the solution conducts electricity
100 of 140
What are intermolecular forces?
there a weak attractive forces between molecules, called intermolecular forces
101 of 140
Many simple molecular substances are insoluble in water. The intermolecular forces between water and these substances are what?
weaker than those between water molecules and molecules of the substance itself
102 of 140
Simple molecular substances dissolve in water if they can form what?
enough strong intermolecular forces with water molecules: hydrogen and oxygen are sparingly soluble (very little dissolves), chlorine + carbon dioxide+ sulfor dioxide + ammonia are soluble, ethanol + ethanoic acid are soluble and sugar is soluble
103 of 140
A giant molecule consists of many atoms. In giant molecules, the atoms are what?
arranged in a regular lattice structure and are joined by strong covalent bonds
104 of 140
What can giant molecular substances be?
non-metal elements such as carbon, compounds such as silica
105 of 140
What do giant molecular substances usually have?
high melting points and high boiling points
106 of 140
What are giant molecular substances at room temperature?
solids. A lot of energy must be transferred to break the many strong covalent bonds during melting and boiling. Giant molecular substances are insoluble in water.
107 of 140
Graphite is used to make electrodes because it conducts electricity. Explain why graphite conducts electricity.
A carbon atom can form four covalent bonds. But in graphite each carbon atom only forms three covalent bonds. The non-bonding outer electrons become delocalised. This means they can move through the structure, so graphite conducts electricity.
108 of 140
What are Graphene and fullerenes forms of?
carbon that exists as giant molecules
109 of 140
What is Graphene?
Graphene is a giant molecular substance. Its structure resembles a single layer of graphite: each carbon atom is covalently bonded to three other carbon atoms and it has a regular lattice structure
110 of 140
What do fullerences resemble?
a sheet of graphene rolled to form hollow balls often called buckyballs and hollow tubes called carbon nanotubes
111 of 140
materials made from buckyballs conduct electricity because they have delocalised electrons and are what?
soft when in the solid state because they have weak intermolecular forces
112 of 140
Nanotubes have closed ends or open ends. They can be several mm long. Nanotubes can do what and are what?
can conduct electricity because they have delocalised electrons and are very strong because the structure has many strong covalent bonds
113 of 140
What are polymers?
Polymers are large molecules made from many smaller molecules, called monomers, joined together
114 of 140
Graphene conducts electricity:
the non-bonding outer shell
115 of 140
What is the appearance of metals?
shiny
116 of 140
What is the appearance of non-metals?
dull
117 of 140
What is the electrical conduction of metals?
good conductors
118 of 140
What is the electrical conduction of non-metals?
poor conductors
119 of 140
What is the density of metals?
high
120 of 140
What is the density of non-metals?
low
121 of 140
What is the melting point of metals?
high
122 of 140
What is the melting points of non-metals?
low
123 of 140
Describe what a metal has?
consists of a giant lattice of positively charged metal ions and has a "sea" of delocalised electrons. The delocalised electrons come from the outer shells of the atoms.
124 of 140
What are Metallic bonds?
are strong electrostatic forces of attraction between positive metal ions and delocalised electrons
125 of 140
metals are what?
malleable- they can be pressed into shape without shattering
126 of 140
non-metals are what?
brittle in the solid state- they shatter when bent or hit
127 of 140
According to the law of conservation of mass, the total mass of reactants and products stays constant during a chemical reaction. The total mass before and after a reaction is what?
the same
128 of 140
What is a closed system?
is a situation in which no substance can enter or leave during a reaction
129 of 140
What do closed systems include?
reactions in a sealed container such as a flask fitted with a bung and precipitation reactions in a beaker
130 of 140
In a precipitation reaction, two soluble reactants form an insoluble product which is?
the precipitate
131 of 140
What is a non-closed system?
is a situation in which substances can enter or leave during a reaction
132 of 140
What does a non-closed systems include ?
reactions in a open flask, where a substance in the gas state may enter or leave
133 of 140
Mass is conserved, but you will observe the following:
the mass of a reactive metal increases if it is heated in air this is because oxygen atoms combine with metal ions to form a metal oxide.
134 of 140
The mass of a reactive non-metal or fuel decreases if it is what?
heated in air. This is because products in the gas state escape from the container
135 of 140
The mass of a metal carbonate decreases if it is what?
heated. This is because carbon dioxide gas is produced and this escapes from the container
136 of 140
What is a Solution?
is a mixture of a solute in a solvent
137 of 140
What is the Solute?
is the substance that dissolves
138 of 140
What is the Solvent?
is the substance that the solute dissolves in
139 of 140
How do you calculate concentration?
concentration= mass of solute (g) divided by volume of solution (dm^3)
140 of 140

Other cards in this set

Card 2

Front

What is meant by the term ion?

Back

An ion is a charged particle formed when an atom, or group of atoms, loses or gains electrons

Card 3

Front

what is a compound?

Back

Preview of the front of card 3

Card 4

Front

what is an atom?

Back

Preview of the front of card 4

Card 5

Front

what is a molecule?

Back

Preview of the front of card 5
View more cards

Comments

No comments have yet been made

Similar Science resources:

See all Science resources »See all PAPER 1+2 resources »