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chem 20 > unit A- topic one > Flashcards

unit A- topic one Flashcards

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1
Q

matter

A

anything that has mass and takes up space

everything is made up of matter

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2
Q

physical properties

A

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

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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)

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4
Q

chemical properties

A

what happens when it reacts

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5
Q

elements

A

things found in the periodic table

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6
Q

diatomic

A

two similar atoms bonded together (BrINClHOF)

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7
Q

polyatomic

A

multiple similar atoms bonded together

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8
Q

polyatomic and diatomic are

A

non-metals

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9
Q

compound

A

composed of at least 2 of the same elements

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10
Q

electrons (charge and location)

A

negative, outside the nucleus

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11
Q

protons (charge and location)

A

positive, inside the nucleus

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12
Q

neutrons (charge and location)

A

no charge, inside the nucleus

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13
Q

atomic number=

A

protons

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14
Q

neutrons=

A

atomic number- protons

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15
Q

atomic mass=

A

neutrons + protrons

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16
Q

protons=

A

electrons (unless it’s an ION)

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17
Q

in an atom…

A

atomic mass = protons = electrons

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18
Q

net charge

A

the difference between electrons and protons

the charge of the atom, is it an ION?

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19
Q

group

A

vertical columns, easy way to find the valence electron number

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20
Q

period

A

horizontal rows, also determine the amount of electron levels

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21
Q

bohr model

A

electrons have definite orbital levels, and includes all energy levels

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22
Q

energy levels

A

2
8
8
the ‘rings’ that electrons rotate around

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23
Q

valence electrons

A

the outer ring in the ‘bohr model’

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24
Q

lewis model

A

shows only the valence electrons

-less crowded, more efficient

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25
Q

bonding electrons

A

are single electrons. on their own in electron levels

they are able to bond with other elements

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26
Q

lone pair

A

a pair of electrons

cannot bond

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27
Q

bonding capacity

A

the amount of bonding electrons, or opportunities to bond

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28
Q

elements found in the higher groups are..

A

not good at bonding since they are filled with lone pairs (energy levels are full)

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29
Q

easier to get rid of

A

electrons in the valence shells

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30
Q

metals tend to

A

give away electrons and be positive (less filled valence electrons)

31
Q

nonmetals tend to

A

except electrons and become negative (almost filled valence electrons)

32
Q

transition metals tend to

A

be confusing and follow a different order

33
Q

ION

A

an atom that gives away or receives electrons, throws off the balanced net charge

34
Q

atomic form

A

neutral, net charge of 0

35
Q

ionic form

A

net charge is positive or negative

36
Q

cation

A

positively charged IONS, have given away electrons

-nonmetals name ends with IDE

37
Q

anion

A

negatively charged IONS, have gained electrons

38
Q

naming order

A

metals first then nonmetals

39
Q

left of periodic table

A

metals and positive

40
Q

right side of periodic table

A

nonmetals and negative

41
Q

physical properties of metals

A
  • shiny
  • malleable
  • ductile
  • conduct electricity
42
Q

physical properties of nonmetals

A
  • dull
  • brittle when solid
  • poor conductors of electricity
43
Q

group 1

A

alkali metals

very reactive, one electron in valence shell and ION+1

44
Q

group 2

A

alkaline earth metals

quite reactive, 2 valence electrons, ION+2

45
Q

group 17

A

halogens

very reactive nonmetals, 7valence electrons, ION-1

46
Q

group 18

A

Nobel gases

very nonreactive, 0 electrons to give or take, full valence electrons

47
Q

reactivity revolves

A

around how little electrons need to be gained or removed

48
Q

electronegativity

A

how attracted is the nucleus to a pair of bonding electrons

49
Q

metals loosing electrons means

A

lower electronegativity

50
Q

nonmetals gaining electrons means

A

higher electronegativity

51
Q

size of the atom =

A

less attraction and electronegativity

52
Q

pure covalent (elecneg)

A

zero electronegativity

53
Q

polar covalent (elecneg)

A

low electronegativity

54
Q

ionic (elecneg)

A

high electronegativity

55
Q

ionic bonding

A

is not literally bonding, just strongly associated

56
Q

crystal lattice

A

solid very stable structure, formed by ionic compoounds

57
Q

ratio of ions

A

to show that there is more than just one atom of each in the compound

58
Q

how does dissolving work

A 
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
Q

exothermic

A

explosion, releases heat

60
Q

endothermic

A

absorbs heat, needs energy

61
Q

tempature

A

the energy particles, and how fast their moving

62
Q

metallic bond

A

ability to share electrons/keep sharing, due to how close molecules are in metals
creating a glue/strong definite structure

63
Q

what is essential for conductivity

A

a charge and a motion

64
Q

coulombs law

A

the higher the lattice energy, stronger the ionic bond

=less soluble in water

65
Q

how can compounds be MORE ionic?

A
  • creates a tighter connection when two molecules have a larger difference of electronegativity
  • the closer a molecule, the greater the connection (magnets)
66
Q

lattice energy

A

the strength of the bonds in ionic compounds

more ionic = more lattice energy

67
Q

covalent bond

A

electrons are shared between two atoms

68
Q

electronegativity difference of 0.0-2.0

A

covalent bonds (equal and unequal)

69
Q

electronegativity difference of 2.0 to 4.0

A

ionic bonds

70
Q

polar covalent

A

covalent that is slightly unequal

71
Q

what if its in the between of the differences

A

look to see if it’s metal + nonmetals, which will show if its ionic or not

72
Q

boiling points show..

A

how strong are the bonds
high BP = high bond (more electrons)
low BP = low bonds

73
Q

how do you find the size of an atom

A

-energy levels

74
Q

why are ionic compounds solid?

A

formed in large lattices/attracted/fused by oppositely charged IONS

chem 20 (7 decks)

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