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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
Those a solid have attractive forces?
Yes
25
The shape of a liquid is....
Indefinite
26
The volume of a solid is...
definite
27
The volume of a liquid is...
Definite
28
Do liquids have attractive forces?
Yes
29
The shape of a gas is...
Indefinite
30
The volume of a gas is...
Indefinite
31
Do gases have attractive forces
No
32
List the four postulates of Dalton's atomic theory.
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.
33
Describe rutherford's experiment
- 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.
34
Location, charge, and mass in amu of the neutron.
Nucleus , 0, 1
35
Location, charge, and mass in amu of the electron.
Outside, negative, 1/1840
36
Location, charge, and mass in amu of the proton.
Nucleus, positive, 1
37
How do u get the mass number?
Protons+neutrons
38
Which particles have the same number unless it is an isotope?
Atomic number Protons Electrons
39
Who do you find the amount of neutrons?
Mass number-protons
40
Atoms of the same element with the same number of protons, but different mass numbers and different numbers of neutrons
Isotopes
41
Equation to find the average atomic mass
(Mass first isotope) x % abundance/100 + (Mass second isotope) x %abundance/100
42
Alpha decay equation
4 He 2
43
Beta decay equation
0 e -1
44
Gamma decay equation
0 Y 0
45
The number of wave cycles that pass a given point per unit of time. Unit.
Frequency | Hz, 1/s, s-1
46
Distance between crests. Unit.
Wavelength | m
47
Minimum amount of energy that can be gained or lost by an atom.
Quanta
48
Three-dimensional region around the nucleus in which an electron moves and is found 90% of the time.
Orbital
49
What happens when electrons jump to higher energy levels?
Atom absorbs energy
50
What happens when electrons fall from higher energy levels to lower energy levels?
Atoms releases energy
51
Speed of light equation.
C=hv
52
Photon energy equation
E=hv
53
Published periodic table, organized elements with similar chemical and physical properties and increasing atomic mass.
Mendeleev
54
Arranged periodic table in order of increasing atomic number.
Moseley
55
Column on the periodic table
Group
56
Across/rows on the periodic table
Period
57
Estimated as half the distance between the nuclei of 2 like atoms of the same element when atoms are joined.
Atomic radii
58
Energy needed to remove an electron from an atom.
Ionizaton energy
59
Ability of an Atom of an element to attract electrons when the Atom is In a compound.
Electronegativity
60
Total charge of all protons in the nucleus
Nuclear charge
61
Energy levels in an atom
Shells
62
Inner level electrons that interfere or shield the valence electrons from the nucleus.
Shielding
63
What particle determines most of the properties of elements?
Electrons
64
What happens to electrons in an ionic compound?
They are transferred
65
What happens to electrons in a covalent bon?d
They are shared
66
Atoms will gain or lose electrons to acquire a full set of 8 valence electrons.
Octet rule
67
What does VSEPR mean?
Valence shell electron pair repulsion
68
Molecule has H-F, H-O, or H-N
Hydrogen bonding
69
Caused by momentary dipoles of constantly moving electrons between nonpolar molecules
Dispersion forces
70
Dependent on the number of electrons, more electrons stronger forces
Dipole-dipole forces
71
How can you identify a polar molecule?
- Have to have at least one polar bond | - polar bonds can't cancel
72
Five reaction types
``` Synthesis Combustion Decomposition Single replacement double replacement ```
73
What happens to the nuclear charge when it moves across the periodic table?
Increases
74
What happens to the nuclear charge when it moves down the periodic table?
Increases but cancels out
75
What happens to shells and shielding when it moves across the periodic table?
It's constant
76
What happens to the shells and shielding when it moves down the periodic table?
Increases
77
What happens to the atomic radius when it moves across the periodic table?
Decreases
78
What happens to the atomic radius when it moves down the periodic table?
Increases
79
What happens to the ionic size when it moves across the periodic table?
Decrease
80
What happens to the ionic size when it moves down the periodic table?
Increases
81
What happens to the ionization energy when it moves across the periodic table?
Increases
82
What happens to the ionization energy when it moves down the periodic table?
Decreases
83
What happens to the electronegativity when it moves across the periodic table?
Increases
84
What happens to the electronegativity when it moves down the periodic table?
Decreases
85
What is the relationship between bond strength and bond length?
They are inversely proportional
86
What is a precipitate?
Formation of a solid in a chemical reaction

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