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flashcards! > H.Chemistry Final > Flashcards

H.Chemistry Final Flashcards

0
Q

SI unit of mass and it’s symbol.

A

Kilograms

Kg

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1
Q

SI unit of length and it’s symbol.

A

Meter

m

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2
Q

SI unit of time and it’s symbol.

A

Seconds

s

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3
Q

SI unit of temperature and it’s symbol.

A

Kelvin

K

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4
Q

SI unit of volume and it’s symbol.

A

Cubic meter

m^3

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5
Q

SI unit of density and it’s symbol.

A

Kilogram per cubic meter

Kg/m^3

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6
Q

Which of the six SI units are derived units?

A

Volume and density

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7
Q

Equation for converting Celsius to kelvin

A

K=t(c)+273.15

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8
Q

Equation for converting Kelvin to Celsius

A

C=t(k)-273.15

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9
Q

Tells how close the individual measurements are to each other.

A

Precision

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10
Q

Describes how close the measurement is to the accepted value

A

Accuracy

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11
Q

Proposed explanation for an observation

A

Hypothesis

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12
Q

Tested explanation for a broad set of observations.

A

Theory

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13
Q

Standard use for comparison

A

Control

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14
Q

Variable that is manipulated

A

Independent variable

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15
Q

Variable that is observed, responds to independent variable.

A

Dependent variable

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16
Q

Equation of the error and percent error

A

Error=experimental-accepted

Percent error= error/accepted x 100

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17
Q

Ability of a substance to undergo a specific chemical change. Examples.

A

Chemical property

  • decomposition
  • rust
  • acid
  • water
  • combustion
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18
Q

Quality of a substance that can be observed without changing the substances composition.Example.

A

Physical property

  • hardness
  • color
  • conductivity
  • malleability
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19
Q

Change that produces matter with a different result than the original matter. Examples.

A

Chemical change

  • color change
  • light or energy involved
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20
Q

Properties of a material change, but the composition of the material doesn’t.

A

Physical change

  • dissolving
  • changes in state
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21
Q

Depends of the type in a sample, NOT the amount of matter.

A

Intensive property

  • density
  • absorbency
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22
Q

Dependent upon the amount of matter in a sample.examples.

A

Extensive property

  • mass
  • volume
  • length
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23
Q

The shape of a solid is…

A

Definite

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24
Q

Those a solid have attractive forces?

A

Yes

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25
Q

The shape of a liquid is….

A

Indefinite

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26
Q

The volume of a solid is…

A

definite

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27
Q

The volume of a liquid is…

A

Definite

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28
Q

Do liquids have attractive forces?

A

Yes

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29
Q

The shape of a gas is…

A

Indefinite

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30
Q

The volume of a gas is…

A

Indefinite

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31
Q

Do gases have attractive forces

A

No

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32
Q

List the four postulates of Dalton’s atomic theory.

A
  1. All elements are composed of tiny indivisible particles called atoms.
  2. Atoms of the same element are identical. The atoms of one element are different from those of any other element.
  3. Atoms combine in simple whole # ratios.
  4. In a reaction, atoms are rearranged but they are never changed into atoms of another element as a result of a chemical reaction.
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33
Q

Describe rutherford’s experiment

A
  • concluded there must be a particle in the nucleus carrying a charge equal but opposite of the electron that was called a proton.
  • concluded that the atoms was mostly empty space.
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34
Q

Location, charge, and mass in amu of the neutron.

A

Nucleus , 0, 1

35
Q

Location, charge, and mass in amu of the electron.

A

Outside, negative, 1/1840

36
Q

Location, charge, and mass in amu of the proton.

A

Nucleus, positive, 1

37
Q

How do u get the mass number?

A

Protons+neutrons

38
Q

Which particles have the same number unless it is an isotope?

A

Atomic number
Protons
Electrons

39
Q

Who do you find the amount of neutrons?

A

Mass number-protons

40
Q

Atoms of the same element with the same number of protons, but different mass numbers and different numbers of neutrons

A

Isotopes

41
Q

Equation to find the average atomic mass

A

(Mass first isotope) x % abundance/100
+
(Mass second isotope) x %abundance/100

42
Q

Alpha decay equation

A

4
He
2

43
Q

Beta decay equation

A

0
e
-1

44
Q

Gamma decay equation

A

0
Y
0

45
Q

The number of wave cycles that pass a given point per unit of time. Unit.

A

Frequency

Hz, 1/s, s-1

46
Q

Distance between crests. Unit.

A

Wavelength

m

47
Q

Minimum amount of energy that can be gained or lost by an atom.

A

Quanta

48
Q

Three-dimensional region around the nucleus in which an electron moves and is found 90% of the time.

A

Orbital

49
Q

What happens when electrons jump to higher energy levels?

A

Atom absorbs energy

50
Q

What happens when electrons fall from higher energy levels to lower energy levels?

A

Atoms releases energy

51
Q

Speed of light equation.

A

C=hv

52
Q

Photon energy equation

A

E=hv

53
Q

Published periodic table, organized elements with similar chemical and physical properties and increasing atomic mass.

A

Mendeleev

54
Q

Arranged periodic table in order of increasing atomic number.

A

Moseley

55
Q

Column on the periodic table

A

Group

56
Q

Across/rows on the periodic table

A

Period

57
Q

Estimated as half the distance between the nuclei of 2 like atoms of the same element when atoms are joined.

A

Atomic radii

58
Q

Energy needed to remove an electron from an atom.

A

Ionizaton energy

59
Q

Ability of an Atom of an element to attract electrons when the Atom is In a compound.

A

Electronegativity

60
Q

Total charge of all protons in the nucleus

A

Nuclear charge

61
Q

Energy levels in an atom

A

Shells

62
Q

Inner level electrons that interfere or shield the valence electrons from the nucleus.

A

Shielding

63
Q

What particle determines most of the properties of elements?

A

Electrons

64
Q

What happens to electrons in an ionic compound?

A

They are transferred

65
Q

What happens to electrons in a covalent bon?d

A

They are shared

66
Q

Atoms will gain or lose electrons to acquire a full set of 8 valence electrons.

A

Octet rule

67
Q

What does VSEPR mean?

A

Valence shell electron pair repulsion

68
Q

Molecule has H-F, H-O, or H-N

A

Hydrogen bonding

69
Q

Caused by momentary dipoles of constantly moving electrons between nonpolar molecules

A

Dispersion forces

70
Q

Dependent on the number of electrons, more electrons stronger forces

A

Dipole-dipole forces

71
Q

How can you identify a polar molecule?

A
  • Have to have at least one polar bond

- polar bonds can’t cancel

72
Q

Five reaction types

A 
Synthesis
Combustion
Decomposition
Single replacement 
double replacement
73
Q

What happens to the nuclear charge when it moves across the periodic table?

A

Increases

74
Q

What happens to the nuclear charge when it moves down the periodic table?

A

Increases but cancels out

75
Q

What happens to shells and shielding when it moves across the periodic table?

A

It’s constant

76
Q

What happens to the shells and shielding when it moves down the periodic table?

A

Increases

77
Q

What happens to the atomic radius when it moves across the periodic table?

A

Decreases

78
Q

What happens to the atomic radius when it moves down the periodic table?

A

Increases

79
Q

What happens to the ionic size when it moves across the periodic table?

A

Decrease

80
Q

What happens to the ionic size when it moves down the periodic table?

A

Increases

81
Q

What happens to the ionization energy when it moves across the periodic table?

A

Increases

82
Q

What happens to the ionization energy when it moves down the periodic table?

A

Decreases

83
Q

What happens to the electronegativity when it moves across the periodic table?

A

Increases

84
Q

What happens to the electronegativity when it moves down the periodic table?

A

Decreases

85
Q

What is the relationship between bond strength and bond length?

A

They are inversely proportional

86
Q

What is a precipitate?

A

Formation of a solid in a chemical reaction

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