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Chemistry 101 > Chapter 1 > Flashcards

Chapter 1 Flashcards

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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)

A

isolated oxygen from the compound mercury oxide

25
Q

Chemical Formula

A

standard formula for writing chemical transformations (lists the symbols of its constituent elements and uses subscripts to indicate the number of atoms each)

26
Q

Chemical equation

A

substance undergoing change –> substances being formed

27
Q

Antoine Lavoisier (1743-1794)

A

oxygen is the key substance in combustion
- law of mass conservation

28
Q

Law of mass conservation

A

mass 1 –> mass 2 + mass 3

29
Q

Joseph Proust (1754-1826)

A

law of definite proportions

30
Q

Law of definite proportions

A

different samples of pure chemical compund always contain the same proportion of elements by mass

31
Q

John Dalton

A

law of multiple proportions

32
Q

Law of multiple proportions

A

elements can combine in many different ways (making chemical compounds) with mass ratios that one simple, whole-number multiple of each other

33
Q

Dalton’s Theory of Matter (4 points)

A

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
Q

JJ Thomson

A

Used cathode ray tubes (CRTs) –> electrons

35
Q

Electrons

A

tiny negatively charged particles

36
Q

Thomson’s reasoning on amount of deflection (3 points)

A

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
Q

alpha particles

A

come off of naturally occuring radioactive elements (7000 times larger than electrons with positive charge)

38
Q

nucleus

A

central core of atoms where mass is concentrated

39
Q

protons

A

positive particle that makes up part of the nucleus

40
Q

neutrons

A

particle with no charge that make up part of the nucleus (similar to the mass of protons)

41
Q

atomic number (Z)

A

number of protons in the atom’s nucleus (number of electrons around an atom’s nucleus)

42
Q

mass number (A)

A

number of protons (z) + number or neutrons (n)

43
Q

Isotopes

A

atoms with the same atomic numbers, but different mass numbers (ex. hydroged)

44
Q

Unified atomic mass unit (u)

A

1/12 of the mass of a carbon atom

45
Q

atomic mass

A

the mass of a specific atom

46
Q

atomic weight

A

the wighted average of the atomic masses of the elements naturally occurring isotopes

47
Q

Mole (mol)

A

unit used for when there are super big numbers of atoms (visible amount) –> contains Avogadro’s number of atoms

48
Q

molar mass

A

mass in grams of any element (numerically equal to its atomic weight)

49
Q

Avogadro’s Number

A

One mole of any element = 6.022 141 x 10^23 atoms

50
Q

nuclear chemistry

A

the study of properties and changes of atomic nuclei

51
Q

Nuclear equation

A

the element symbols represent only the nuclei of atoms (subscript only represents the number of nuclear charges (protons)

52
Q

Radioactive

A

(element/atoms) undergoes a spontaneous change (nuclear decay) and emits some form of radiation

53
Q

Alpha radiation

A

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
Q

Radioisotopes

A

heavy radioactive isotopes (ex. Uranium-238)

55
Q

Nucleons

A

The total number of protons and neutrons

56
Q

Beta Radiation

A

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
Q

Gamma Radiation

A

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
Q

Positron emission

A

occurs when a proton in the nucleus changes into a neutron plus an ejected positron

59
Q

electron capture

A

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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