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Chemistry 101 > Chapter 1 > Flashcards

Chapter 1 Flashcards

(59 cards)

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1
Q

element

A

fundamental substance that can’t be chemically changed or broken down into anything simpler (there are 118)

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2
Q

hydrogen

A

75% of the observed mass in the universe

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3
Q

oxygen and silicon

A

together account for 75% of the earth’s crust

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4
Q

oxygen, carbon, and hydrogen

A

more than 90% of the human body

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5
Q

periods

A

the 7 horizontal rows

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6
Q

groups

A

the 18 vertical columns (contain elements with similar chemical properties)

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7
Q

main group elements

A

carbon, oxygen, hydrogen, nitrogen, and phosphorous

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8
Q

transition metal groups (examples)

A

labeled B –> in the middle of the table (ex. iron, copper, zinc, and gold)

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9
Q

inner transition metal groups

A

the 14 groups on the bottom of the table

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10
Q

property (seven examples)

A

any characteristic that can be used to describe of identify matter
- volume
- amount
- odor
- temperature
- melting pint
- solubility
- chemical behavior

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11
Q

Intensive properties (two/three examples)

A

have values that don’t depend on the amount of sample
- temperature (ex. ice cubes and icebergs have the same melting point)
- melting point

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12
Q

Extensive properties (two examples)

A

have values that do depend on the sample size
- length
- volume

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13
Q

physical properties (8 examples)

A

characteristics that don’t involve a change in a sample’s chemical makeup
- temperature
- color
- melting point
- electrical conductivity
- amount
- odor
- solubility
- hardness

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14
Q

chemical properties

A

characteristics that do involve a change in a sample’s chemical makeup
- rusting (of iron)
- combustion (of gasoline)
- tarnishing (of silver)
- hardening (of cement)

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15
Q

group 1A

A

Alkali Metals –> react rapidly and violently to water (forming products that are highly alkaline)

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16
Q

group 2A

A

Alkaline Earth metals –> less reactive than 1A (never found in nature in their pure state)

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17
Q

group 7A

A

Halogens –> colorful and corrosive metals

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18
Q

group 8A

A

Noble gases

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19
Q

metals (four identifiable features)

A
  • largest category of elements (left side of the table)
  • identifiable appearance (silver shine, solid at room temperature (except mercury), malleable, conductors of heat and electricity)
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20
Q

nonmetals

A

right side of periodic table (except hydrogen)
- 11 Gases
-1 liquid (Bromine)
- 5 solids at room temperature

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21
Q

Semimetals

A

semi because they are brittle and poor conductors (ex. silicon because its conductivity is somewhere between a metal and insulator)

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22
Q

Rober Boyle

A

credited for being the first to study chemistry as a separate intellectual discipline

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23
Q

chemical compounds

A

substances made of the atoms of multiple elements

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24
Q

Joseph Preistly (1733-1804)

Study These Flashcards
A

isolated oxygen from the compound mercury oxide

25
Chemical Formula
standard formula for writing chemical transformations (lists the symbols of its constituent elements and uses subscripts to indicate the number of atoms each)
26
Chemical equation
substance undergoing change --> substances being formed
27
Antoine Lavoisier (1743-1794)
oxygen is the key substance in combustion - law of mass conservation
28
Law of mass conservation
mass 1 --> mass 2 + mass 3
29
Joseph Proust (1754-1826)
law of definite proportions
30
Law of definite proportions
different samples of pure chemical compund always contain the same proportion of elements by mass
31
John Dalton
law of multiple proportions
32
Law of multiple proportions
elements can combine in many different ways (making chemical compounds) with mass ratios that one simple, whole-number multiple of each other
33
Dalton's Theory of Matter (4 points)
1) Elements are made up of tiny particles called atoms; 2) Each element is characterized by the mass of its atoms; 3) The chemical combination of elements to make different chemical compounds occurs when atoms bond together in small whole number ratios; 4) Chemical reactions only rearrange how atoms are combined in chemical compounds, the atoms themselves don't change.
34
JJ Thomson
Used cathode ray tubes (CRTs) --> electrons
35
Electrons
tiny negatively charged particles
36
Thomson's reasoning on amount of deflection (3 points)
1) stronger magnet = stronger deflection; 2) larger charge for each particle = more interaction with magnetic/electric field --> greater deflection; 3) the lighter (mass) the particle = the greater the deflection
37
alpha particles
come off of naturally occuring radioactive elements (7000 times larger than electrons with positive charge)
38
nucleus
central core of atoms where mass is concentrated
39
protons
positive particle that makes up part of the nucleus
40
neutrons
particle with no charge that make up part of the nucleus (similar to the mass of protons)
41
atomic number (Z)
number of protons in the atom's nucleus (number of electrons around an atom's nucleus)
42
mass number (A)
number of protons (z) + number or neutrons (n)
43
Isotopes
atoms with the same atomic numbers, but different mass numbers (ex. hydroged)
44
Unified atomic mass unit (u)
1/12 of the mass of a carbon atom
45
atomic mass
the mass of a specific atom
46
atomic weight
the wighted average of the atomic masses of the elements naturally occurring isotopes
47
Mole (mol)
unit used for when there are super big numbers of atoms (visible amount) --> contains Avogadro's number of atoms
48
molar mass
mass in grams of any element (numerically equal to its atomic weight)
49
Avogadro's Number
One mole of any element = 6.022 141 x 10^23 atoms
50
nuclear chemistry
the study of properties and changes of atomic nuclei
51
Nuclear equation
the element symbols represent only the nuclei of atoms (subscript only represents the number of nuclear charges (protons)
52
Radioactive
(element/atoms) undergoes a spontaneous change (nuclear decay) and emits some form of radiation
53
Alpha radiation
consists of a stream of particles that are repelled by a positively charged electrode (attracted by a negatively charged electrode) and have a mass to charge ratio identifying them as helium nuclei --> alpha particles therefore have 2 protons and 2 neutrons
54
Radioisotopes
heavy radioactive isotopes (ex. Uranium-238)
55
Nucleons
The total number of protons and neutrons
56
Beta Radiation
Consists of a stream of particles that are attracted to a positive electrode (repelled by a negative electrode) and have a mass to charge ratio identifying them as electrons - occurs when a neutron spontaneously decays into a proton and an electron (which is then ejected (ex. Iodine-131))
57
Gamma Radiation
Unaffected by electric and magnetic fields and has no mass --> basically electromagnetic radiation of a very high energy --> typically accompanies alpha and beta radiation emission (not typically shown when writing nuclear equations)
58
Positron emission
occurs when a proton in the nucleus changes into a neutron plus an ejected positron
59
electron capture
a process in which the nucleus capture one of the surrounding electrons in an atom (converting a proton into a neutron)

Chemistry 101 (3 decks)

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