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Chem 16 > Matter > Flashcards

Matter Flashcards

1
Q

the study of matter (composition &
properties), the changes that it
undergoes, and the energy associated
with those changes

A

Chemistry

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2
Q

Chemistry is the study of * (composition &
properties), the * that it
undergoes, and the * associated
with those *

A

matter, changes, energy, changes

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3
Q

Chemistry at three levels:
M -
P -
S -

A

Macroscopic * - observe
Particulate * - imagine
Symbolic * - represent

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4
Q

a hot ionized gas consisting of approximately equal
numbers of positively charged ions and negatively
charged electrons; it is strongly influenced by …

A

plasma, electric and magnetic fields

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5
Q

According to democritus (400 BC), matter is made up of

A

atoms

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6
Q

5 main elements of Earth’s crust

A

Oxygen, Silicon, Aluminum, Iron, Calcium… other

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7
Q

3 main elements of human body

A

Carbon, Oxygen, Hydrogen

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8
Q

Uuo 118

113, 115, 117,

A

Ununoctium

Ununtrium, Ununpentium, Ununseptium

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9
Q

Formed when two or more atoms join together chemically

A

molecule

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10
Q

a molecule that contains at least two different elements

A

compounds

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11
Q

Properties of matter:
physical/chemical: consider the *
intensive/extensive: consider the *

A

change in composition

in the amount of substance

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12
Q

can be observed without changing a

substance into another substance

A

physical properties

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13
Q

color, odor, density, length, melting point,

boiling point, hardness, etc.

A

physical properties

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14
Q

Examples of physical properties

A

color, odor, density, length, melting point,

boiling point, hardness, etc.

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15
Q

individual components of a *

may be separated by *

A

mixture, physical properties

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16
Q 
Physical Property vs Means of Separation
density
boiling point
state of matter
intermolecular forces
vapor pressure
magnetism
solubility
A 
decantation, centrifugation
distillation
filtration
chromatography
evaporation
magnets
filtration
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17
Q 
Means of Separation vs Physical Property
decantation, centrifugation
distillation
filtration
chromatography
evaporation
magnets
filtration
A 
density
boiling point
state of matter
intermolecular forces
vapor pressure
magnetism
solubility
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18
Q

only observed when a substance is changed into

another substance

A

Chemical Properties

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19
Q

flammability,
coordination number,
radioactivity, oxidation

A

Chemical Properties

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20
Q

Example of Chemical Properties

A

flammability,
coordination number,
radioactivity, oxidation

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21
Q

independent of the amount of the substance that is present; important for * a substance

A

Intensive properties; identifying

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22
Q

depend upon the amount of the substance present

A

extensive properties

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23
Q

Example of extensive properties

A

Volume, mass, size, weight, length, energy?

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24
Q

Example of intensive properties

A

Boiling point, color, temperature, luster, hardness

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25
Q

changes in matter that do not change
the composition of a substance
examples include changes of state, temperature, and volume

A

Physical change

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26
Q

result in new substances

examples include combustion, oxidation, and decomposition

A

CHEMICAL CHANGES

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27
Q

Example of physical change

A

changes of state, temperature, and volume

28
Q

Example of chemical change

A

combustion, oxidation, and decomposition

29
Q

the energy of motion; magnitude depends

on an object’s mass (m) and its velocity (v)

A

Kinetic Energy

30
Q

depends on an object’s relative position

with respect to other objects

A

POTENTIAL ENERGY

31
Q

in science, a * is collection of
quantitative or numerical data that describes a
property of an object or event

A

measurement

32
Q

in science, a measurement is collection of

  • that describes a
  • of an object or event. Measurement is made by comparing a quantity with a …
A

quantitative or numerical data, property

standard unit.

33
Q

in chemistry, we use the *
in measuring different quantities/properties
measurement =

A

SI units

number + unit

34
Q

STANDARD UNITS =

A

Système International
d’Unités (SI)
(The International System of
Units)

35
Q
  • a measure of the amount of material in an object
    SI base unit = kilogram; metric base unit = gram
  • a measure of distance
    base unit = meter
A

MASS

LENGTH

36
Q
  • in general usage, it is the “hotness and coldness” of
    an object that determines the direction of heat flow*
    base unit = kelvin
A

Temperature

37
Q

K —–> °C CONVERSION | K =

A

°C + 273.15

38
Q

Celsius scale is based on the *

—-> 0 °C is the freezing point of water, while 100 °C is its boiling point

A

properties of water

39
Q
  • is the SI unit of temperature
    –based on the properties of *
    –there are no * Kelvin temperatures
    –the lowest possible temperature is called *
A

Kelvin, gases, negative, absolute zero (0 K)

40
Q

quantities that are calculated from base units

A

derived units

41
Q

quantity that indicates the amount of matter per

unit volume of a sample

A

density

42
Q

percentage of a component in

relation to the total mass of the compound

A

percent composition

43
Q

how closely individual measurements agree

with the correct, or “true,” value

A

ACCURACY

44
Q

measure of how closely individual

measurements agree with one another

A

PRECISION

45
Q

Differentiate accuracy and precision

A

Accuracy refers to how closely individual measurements agree with the correct, or “true,” value while Precision is a measure of how closely individual
measurements agree with one another

46
Q

smallest particle that is

characteristic of a given element

A

Atom

47
Q 
Development of the atomic model
5th Century BC: 
1773: 
1799: 
1800s:
A

DEMOCRITUS AND THE Atomos
Lavoisier’s Law of Conservation of Mass
Proust’s Law of DEFINITE PROPORTIONS
DALTON’S ATOMIC THEORY OF MATTER

48
Q 
Development of the atomic model
DEMOCRITUS AND THE Atomos
Lavoisier’s Law of Conservation of Mass
Proust’s Law of DEFINITE PROPORTIONS
DALTON’S ATOMIC THEORY OF MATTER
A

5th Century BC:
1773:
1799:
1800s:

49
Q 
ideological and philosophical reasoning on the existence of atoms
§ tiny, indivisible particles of matter
called atomos
§ atoms differ in size, shape, and
arrangement in space
§ first theory of atoms
A

Democritus

50
Q

father of modern chemistry
§ observed that matter is
conserved in his experiments

A

ANTOINE LAURENT

LAVOISIER (1743 – 1794)

51
Q

LAW OF CONSERVATION OF

MASS

A

matter is neither created nor

destroyed in a chemical reaction

52
Q

Dans la nature rien ne se crée,

rien ne se perd, tout change.

A

In nature, nothing is created,

nothing is lost, everything changes.

53
Q

each compound always contains the
same elements in a certain definite
proportion and in no other combination

A

LAW OF DEFINITE PROPORTIONS

JOSEPH LOUIS PROUST

54
Q

If two elements A and B combine to form more than one

compound, the masses of B that can combine with a given mass of A are in the *

A

{Law of Multiple Proportions}

ratio of small whole numbers

55
Q

“each element is composed of
unique type of atom which can
combine in different ratios to form
different compounds”

A 
John Dalton (1766 – 1844)
ATOMIC THEORY OF MATTER
56
Q

DALTON’S ATOMIC THEORY
1. Elements are made of extremely small particles called atoms.
2. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties.
3. Atoms cannot be subdivided, created, or destroyed.
In chemical reactions, atoms are combined, separated, or rearranged.
4. Atoms of different elements combine in simple whole-number ratios to form chemical compounds.

A

read

57
Q

1869:
1886:
1897:
1909:

A 
Mendeleev’s PERIODIC TABLE of elements
Goldstein and THE PROTON
JJ Thomson, THE ELECTRON, AND THE PLUM
PUDDING MODEL
Millikan and THE CHARGE OF AN ELECTRON
58
Q 
Mendeleev’s PERIODIC TABLE of elements
Goldstein and THE PROTON
JJ Thomson, THE ELECTRON, AND THE PLUM
PUDDING MODEL
Millikan and THE CHARGE OF AN ELECTRON
A

1869:
1886:
1897:
1909:

59
Q

1911:
1913:
1926:
1932:

A

Rutherford’s NUCLEAR MODEL
Bohr’s PLANETARY model
Schrödinger’s QUANTUM MECHANICAL MODEL
Chadwick and the NEUTRON

60
Q

Rutherford’s NUCLEAR MODEL
Bohr’s PLANETARY model
Schrödinger’s QUANTUM MECHANICAL MODEL
Chadwick and the NEUTRON

A

1911:
1913:
1926:
1932:

61
Q

mass of electron, proton, neutron

A
  1. 11 * 10^-31 kg
  2. 67 * 10^-27 kg
  3. 67 * 10^-27 kg
62
Q

A,z (x)c

A 
A = atomic mass
Z = atomic number
x = element
c = electric charge
63
Q

H-1, H-2, H-3

A

Protium, Deuterium, Tritium

64
Q

are atoms that have the same atomic number (Z)

but different mass numbers (A)

A

ISOTOPES

65
Q

The * of an element is the average of the isotopic masses, weighted according to the naturally occurring abundances of the isotopes of the element

A

atomic mass (weight)

Chem 16 (9 decks)

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