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Chemistry
Molecular & Ionic Compounds
Atomic structure
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Chemistry
Molecular & Ionic Compounds
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42 Terms
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1
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what are atoms
very small particles made up of three main subatomic particles (protons, neutrons and electrons)
2
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where are protons and neutrons found in an atom
in the nucleus (small dense central region)
3
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charge of a proton
\+1
4
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charge of a neutron
0
5
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charge of an electron
\-1
6
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where is the electron found in an atom
outside the nucleus (on shells)
7
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which one is the mass number and the atomic number
8
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why is the nucleus positively charged
it contains positively charged protons and neutral neutrons
9
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why are all atoms neutral
they contain equal numbers of positively charged protons and negatively charged electrons
10
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what is the atomic number
the number of protons in the nucleus
11
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what is the mass number
number of protons plus the number of neutrons in the nucleus
12
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what are elements
substances made up of only type of atom
13
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how to figure out no. of neutrons of an atom
mass no. - atomic no.
14
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what are isotopes
atoms with the same number of protons but different numbers of neutrons
15
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why do isotopes of an element have different masses
due to the different numbers of neutrons in their nuclei
16
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why do isotopes of an element behave the same way in chemical reactions
since the number of electrons determines the way an atom reacts (have same no. of electrons and protons - atomic no.)
17
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what differs or stays the same between isotopes of an atom
different - no. of neutrons
same - no. of electrons and protons
18
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how to figure out no. of protons of an atom
mass no. - no. of neutrons (atomic no. = no. of protons)
19
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order of maximum electronic configuration
2,8,8,2
20
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what do lewis diagrams include
only valence electrons
21
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what are valence electrons
electrons in the outer most shell (highest occupied energy level)
22
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what number of valence electrons is not exceeded
past 8 valence electrons
23
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what electrons are involved in chemical reactions
only valence electrons
24
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what tends to happen when atoms have the same number of valence electrons
they have similar chemical properties
25
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what is the period of a periodic table
the same row across the periodic table
26
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what is the group of a periodic table
same column down the periodic table
27
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how to figure out valence electrons for group 1 and 2
no. of valence electron = group number eg. group 2 has 2 valence electrons
28
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how to figure out valence electrons for group 13 to 18
no. of valence electron = group number - 10 eg. group 17 has 7 valence electrons
29
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what does the number of valence electrons do across a period
increases
30
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what does the number of valence electrons do down a group
remains the same
31
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what are cations
positively charged ions (have fewer electrons than protons)
32
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when do cations form
when atoms or a group of atoms lose electrons
33
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what are anions
negatively charged ions (have more electrons than protons)
34
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what groups of the periodic table are metals found in
groups 1, 2 and 13
35
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what trend do metals usually do (link cations)
tend to lose electrons to form monatomic cations (one atom)
36
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what groups of the periodic table are non-metals found in
groups 15, 16 and 17
37
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what trend do non-metals usually do (like anions)
tend to gain electrons to form monoatomic anions
38
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whats special about group 18 elements
they are unreactive towards most other elements (do not tend to from ions)
39
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what are polyatomic ions
ions that consist of a stable group of atoms with an overall charge eg. NH4
40
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what is the valency of an ion
the magnitude or size of the charge of the ion eg. sodium ion valency is +1
41
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what can transition metals do
can form a range of cations with different valencies eg. copper or iron
42
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what groups are non-metals found
groups 14-17
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