first test Flashcards
(92 cards)
1
Q
Matter
A
anything that has mass and takes up space
2
Q
mass
A
amount of matter that an object contains
3
Q
mass v. Weight
A
weight is the measure of pull of gravity on object and mass is amount of matter the object contains - mass is constant throughout universe and weight is subjective to where you are in the universe
4
Q
Volume
A
the amount of space an object takes up
5
Q
what does matter make up
A
everything
6
Q
how can properties of matter classified?
A
they can be classified as intensive or extensive
7
Q
Extensive Properties
A
extensive property is a property that depends on the amount of matter in a sample, such as mass and volume
8
Q
Intensive Properties
A
property that depends on type of matter in sample, not amount of matter - every sample of a given substance should have the same intensive properties
9
Q
Substance
A
matter that has a uniform and definite composition
10
Q
pure substance
A
contains only one type of matter(is NOT a mixture, one type of element, or compound ) basically only one type of particle
11
Q
Physical property
A
condition or quality of a substance that can be measured or observed while not making any chemical changes to the substance - physical changes are ok
12
Q
examples of physical properties (7)
A
(hardness, color, conductivity, malleability, Density, Melting Point, Solubility)
13
Q
3 states of matter
A
solid liquid gas
14
Q
solid(4)
A
- particles packed close together
- almost in-compressible,
- expands only slightly when heated,
- shape does not depend on shape of container
15
Q
Liquid (5)
A
- particles contact one another but not packed in rigid arranged
- almost incompressible
- expand moderately when heated
- has no independent shape, takes on shape of its container
- it can flow
16
Q
Gas (3)
A
- has indefinite volume and shape
- it is compressible
- Expands greatly when heated
17
Q
Vapor
A
substance in its gaseous state that is ordinarily a liquid or solid at room temperature
18
Q
Physical change
A
some properties of material can change, but composition does not change
19
Q
liquid to gas transition
A
evaporation
20
Q
what are the two types of physical changes?
A
reversible or irreversible
21
Q
gas to liquid transition
A
condensation
22
Q
solid to liquid transition
A
melting
23
Q
liquid to solid transition
A
freezing
24
Q
solid to gas transition
A
sublimation
25
gas to solid transition
deposition
26
mixture
physical blend of two or more substances - can be physically separated into its components
27
what are the two types of mixtures?
heterogeneous and homogenous
28
heterogeneous mixtures
have not uniform composition mixture
29
homogenous mixtures
uniform composition mixture
30
solution
homogenous mixture
31
element
substance that cannot be broken down into simpler substances under normal laboratory conditions - simplest forms of matter
32
compound(3)
-substance that can be separated into simpler substances only by chemical reactions, consist of two or more elements.
- generally properties of compounds are different than that of their component elements.
- specific compound always made up of same elements in same proportion
33
chemical properties
ability of substance to undergo chemical reactions and form new substances - only observed when substance undergoes chemical change and results in change of chemical composition
34
law of conservation of mass
total mass of reactants is always equal to total mass of products, quantity of matter is unchanged
35
Democritus
ancient philosopher, suggested existence of atoms, believed they were indivisible and indetructible
36
Dalton's atomic theory main points(5)
1) Everything is composed of atoms, which are the indivisible building blocks of matter and cannot be destroyed
2) all Atoms of an element are identical
3) the Atoms of different elements vary in size and mass
4)compounds are produced through different whole-number combination of atoms
5)chemical reactions results in rearrangement of atoms in the reactant and product compounds
37
Cathode ray tube
sealed gas tube with near vacuum with two electrodes, when voltage is applied accross them a cathode ray beam occurs
38
cathode rays
stream of electrons travelling from one end of cathode ray to another
39
JJ Thomson's experiemnt
studied cathode ray tubes, believed particles (electrons) must be negative, he said they must be part of all atoms
40
what was JJ Thomson's atom model
plum pudding, which was like a cloudy positive particle with negative electrons in it
41
Milikan's oil drop experiment
measured charge of electron by having an electric field between metal plates, and speed at which oil drops fell in different voltages helped him figure out the charge of an electron
42
Rutherford
proved thomson's model incorrect, used gold foil experiment to show existence of protons and the atomic nucleus
43
Gold Foil Experiment
used beam of positively charged alpha particles(2 protons and 2 neutrons) and shot at very thing piece of gold foil, studied scattering of particles using screen behind foil, he found that the particles rarely were deflected, meaning the positive bodies within the gold atoms in the foil (neuclei) must be really small for them to be hit, most alpha particles passed through gold foil, showing how much of atom must be empty space.
44
conclusions from golf foil experiment(2)
1. volume occupied by atom must consist of large amount of empty space
2. small, relatively heavy, positively charged body (nucleus) must be at the center of every atom
45
Bohr's atomic model
said electrons traveled in orbits around nucleus, and that chemical properties were determined by the number of electrons in the outer orbits
46
chadwik
discovered neutrons with oscilloscope, found they were slightly heavier than protons and had neutral charge
47
purpose of neutrons
to help reduce repulsion between protons to stabilize atom's nucleus
48
quarks
composes protons and neutrons, held together by color force
49
what is the strong force a byproduct of
the color force
50
how are protons and neutrons held together
the strong force (gluons)
51
what is the mass of a neutron/proton (roughly) ?
1.97*10^-24 grams
52
proton
positively charged subatomic particle forming part of nucleus of an atom, determines atomic number of an element
53
neutron
subatomic particle forming part of nucleus, no charge
54
mass of an electron
weigh only 9.11*10^28 grams, usually negligible
55
atomic mass
average masses of isotopes based on their abundance
56
Atomic number
number of protons in an element
57
mass number
number of protons + number of neutrons
58
atomic mass unit
1/12th mass of carbon- 12 atom?
59
mendeleev's periodic table
ordered in terms of relative mass, realized properties of elements related to mass in "periodic" way, arranged them so properties fell together
60
moseley
discovered that energy of x-rays got larger with each element, proposed it was function of positive charge in nucleus, rearranged periodic table to atomic number instead of mass
61
periodic law
states properties of elements recur in systematic way when elements are arranged in order of increasing atomic number
62
horizontal rows in periodic table
periods
63
vertical rows in periodic table
groups
64
how many periods are there in the periodic table
7
65
groups/famlies
arranged so elements in groups have same number of valence electrons
66
valence electrons
electrons in outer most shell, that can be gained or lost in chemical reaction
67
metals
elements that have high electrical conductivity, high luster when clean
68
non-metals
elements that are poor conductors of electricity and are non-lustous when clean
69
metalloids
intermediate properties between those of metals and nonmetals
70
alkali metals
group 1 (IA) of periodic table, shiny, soft, highly reactive metals,
71
Alkali earth metals
belong to group 2 (llA)
alkali earth metals are shiny, silvery white, low density, somewhat reactive
72
general groups in A type elements
metals, non-metals, metalloids
73
transition metals
group B elements, are high density, hard, high melting/boiling points
74
isosagens
belong to group 13 (lllA)
75
tetragens
elements that belong to group 14 (lV) of periodic table
76
Pnictogens
group 15 (VA)
77
Chalcogens
group 16 (VlA)
78
Halogens
Group 17 (VllA) all nonmetals, highly reactive
79
Noble Gases
group 18 (VlllA) all odorless, colorless, and nonmetals
80
types of inner transition metals
lanthanides and actinides
81
lanthanides
period 6, atomic numbers 57-71, known as rare earth metals
82
Actinides
period 7, all radioactive, atomic numbers 89-103,
83
representative elements
elements within groups (lA, llA, lllA, lVA, VA, VlA, VllA, VlllA) - all group A elements
84
who discovered isotopes
Francis Aston discovered that there were three types of hydrogen atoms, called them isotopes
85
isotopes
atoms of same elements with different numbers of neutrons, isotopes still have very similar physical properties
86
half-life
time it takes for half of a sample of an isotope to decay
87
radiocarbon dating
using how much Carbon 14 has deteriorated in an object to tell how old it is
88
radioactive isotopes
isotopes that throw off radiation in an effort to become more stable
89
Alpha radiation
composed of heavy particles, consisting of two protons and two neutrons
90
Beta radiation
consists of electrons
91
gamma radiation
consists of photons
92
isotopes of carbon
carbon 12(98.9), 13(1.1), 14 (<0.1) decreasingly abundant.
