Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

chem 20 > unit A- topic one > Flashcards

unit A- topic one Flashcards

1
Q

matter

A

anything that has mass and takes up space

everything is made up of matter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

physical properties

A

things you can observe -color, texture, size and shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

physical properties states that..

A

as long as certain matter has the same properties it is considered that matter
(physical properties help us distinguish what is what)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

chemical properties

A

what happens when it reacts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

elements

A

things found in the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

diatomic

A

two similar atoms bonded together (BrINClHOF)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

polyatomic

A

multiple similar atoms bonded together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

polyatomic and diatomic are

A

non-metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

compound

A

composed of at least 2 of the same elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

electrons (charge and location)

A

negative, outside the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

protons (charge and location)

A

positive, inside the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

neutrons (charge and location)

A

no charge, inside the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

atomic number=

A

protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

neutrons=

A

atomic number- protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

atomic mass=

A

neutrons + protrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

protons=

A

electrons (unless it’s an ION)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

in an atom…

A

atomic mass = protons = electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

net charge

A

the difference between electrons and protons

the charge of the atom, is it an ION?

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

group

A

vertical columns, easy way to find the valence electron number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

period

A

horizontal rows, also determine the amount of electron levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

bohr model

A

electrons have definite orbital levels, and includes all energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

energy levels

A

2
8
8
the ‘rings’ that electrons rotate around

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

valence electrons

A

the outer ring in the ‘bohr model’

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

lewis model

A

shows only the valence electrons

-less crowded, more efficient

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
bonding electrons
are single electrons. on their own in electron levels | they are able to bond with other elements
26
lone pair
a pair of electrons | cannot bond
27
bonding capacity
the amount of bonding electrons, or opportunities to bond
28
elements found in the higher groups are..
not good at bonding since they are filled with lone pairs (energy levels are full)
29
easier to get rid of
electrons in the valence shells
30
metals tend to
give away electrons and be positive (less filled valence electrons)
31
nonmetals tend to
except electrons and become negative (almost filled valence electrons)
32
transition metals tend to
be confusing and follow a different order
33
ION
an atom that gives away or receives electrons, throws off the balanced net charge
34
atomic form
neutral, net charge of 0
35
ionic form
net charge is positive or negative
36
cation
positively charged IONS, have given away electrons | -nonmetals name ends with IDE
37
anion
negatively charged IONS, have gained electrons
38
naming order
metals first then nonmetals
39
left of periodic table
metals and positive
40
right side of periodic table
nonmetals and negative
41
physical properties of metals
- shiny - malleable - ductile - conduct electricity
42
physical properties of nonmetals
- dull - brittle when solid - poor conductors of electricity
43
group 1
alkali metals | very reactive, one electron in valence shell and ION+1
44
group 2
alkaline earth metals | quite reactive, 2 valence electrons, ION+2
45
group 17
halogens | very reactive nonmetals, 7valence electrons, ION-1
46
group 18
Nobel gases | very nonreactive, 0 electrons to give or take, full valence electrons
47
reactivity revolves
around how little electrons need to be gained or removed
48
electronegativity
how attracted is the nucleus to a pair of bonding electrons
49
metals loosing electrons means
lower electronegativity
50
nonmetals gaining electrons means
higher electronegativity
51
size of the atom =
less attraction and electronegativity
52
pure covalent (elecneg)
zero electronegativity
53
polar covalent (elecneg)
low electronegativity
54
ionic (elecneg)
high electronegativity
55
ionic bonding
is not literally bonding, just strongly associated
56
crystal lattice
solid very stable structure, formed by ionic compoounds
57
ratio of ions
to show that there is more than just one atom of each in the compound
58
how does dissolving work
``` polar water, pulls apart the crystal lattice structure using either ends of the semi charged molecule the positive(hydrogen) pulls at the negative negative(oxygen) pulls at positive ```
59
exothermic
explosion, releases heat
60
endothermic
absorbs heat, needs energy
61
tempature
the energy particles, and how fast their moving
62
metallic bond
ability to share electrons/keep sharing, due to how close molecules are in metals creating a glue/strong definite structure
63
what is essential for conductivity
a charge and a motion
64
coulombs law
the higher the lattice energy, stronger the ionic bond | =less soluble in water
65
how can compounds be MORE ionic?
- creates a tighter connection when two molecules have a larger difference of electronegativity - the closer a molecule, the greater the connection (magnets)
66
lattice energy
the strength of the bonds in ionic compounds | more ionic = more lattice energy
67
covalent bond
electrons are shared between two atoms
68
electronegativity difference of 0.0-2.0
covalent bonds (equal and unequal)
69
electronegativity difference of 2.0 to 4.0
ionic bonds
70
polar covalent
covalent that is slightly unequal
71
what if its in the between of the differences
look to see if it's metal + nonmetals, which will show if its ionic or not
72
boiling points show..
how strong are the bonds high BP = high bond (more electrons) low BP = low bonds
73
how do you find the size of an atom
-energy levels
74
why are ionic compounds solid?
formed in large lattices/attracted/fused by oppositely charged IONS

chem 20 (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions