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H Chemisty I > Exam > Flashcards

Exam Flashcards

1
Q

Base unit

A

Defined unit in a system of measurement that is based on an object or event in the physical world

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2
Q

Second (SI Unit)

A

The physical standard used to define the second is the frequency of the radiation given off by a cesium-133 atom. Time=second(s)

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3
Q

Meter (SI Unit)

A

Length=meter (m) The distance that light travels in a vacuum in 1/299,792,458 of a second. A vacuum exists where space contains no matter

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4
Q

Kilogram (SI Unit)

A

Mass=kilogram (kg) mass is the amount of matter an object contains

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5
Q

Kelvin (SI Unit)

A

Temperature=kelvin (K) Zero kelvin is where all particles are at their lowest possible energy state. Water freezes at 273.15 K and boils at 373.15 K. K=Celsius+273

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6
Q

Derived unit

A

A unit that is defined by a combination of base units

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7
Q

Volume

A

The space occupied by an object (cm^3)

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8
Q

Liter

A

Commonly used to measure the volume of water and beverage containers.

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9
Q

Dimensional analysis

A

A systematic approach to problem solving that uses conversion factors to move, or convert, from one unit to another

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10
Q

Conversion factor

A

A ratio of equivalent values having different units

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11
Q

Accuracy

A

Refers to how close a measured value is to an accepted value.

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12
Q

Precision

A

Refers to how close a series of measurements are to one another

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13
Q

Error

A

Defined as the difference between an experimental value and accepted value

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14
Q

Percent error

A

Expresses error as a percentage of the accepted value

Percent error=(error/accepted value)x100

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15
Q

Density

A

Physical property of matter and is defined as the amount of mass per unit volume.
Density=mass/volume

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16
Q

Graph

A

Visual display of data

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17
Q

Circle graph

A

Useful for showing parts of a fixed whole

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18
Q

Bar graphs

A

Used to show hoe a quantity varies across categories. The quantity being measured appears on the vertical axis (y-axis). The independent variable appears on the horizontal axis (x-axis).

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19
Q

Line graphs

A

Most common in chemistry. The points represent the intersection of data for two variables. The independent variable is plotted on the x-axis. The dependent variable is plotted on the y-axis

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20
Q

Slope

A

Slope=rise/run when the mass of a material is plotted against its volume, the slope of the line represents the material’s density.

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21
Q

Significant figure—adding and subtracting

A

The answer must be rounded to the least precise place

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22
Q

Significant figure—multiplication and division

A

Answer must be rounded to the least number of significant figures in the numbers multiplied or divided

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23
Q

States of matter

A

Physical forms of all matter that exists naturally on Earth

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24
Q

Solid

A

Form of matter that has its own definite shape and volume

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25
Q

Liquid

A

A form of matter that flows, has constant volume, and takes the shape of its container

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26
Q

Gas

A

Form of matter that not only flows to conform to the shape of its container but also fills the entire volume of its container

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27
Q

Physical property

A

Characteristic of matter that can be observed or measured without changing the sample’s composition.
Examples: density, color, odor, hardness, melting point, boiling point

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28
Q

Extensive properties

A

Physical properties that are dependent on the amount of substance present.
Examples: mass, length, volume

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29
Q

Intensive properties

A

Physical properties that are independent of the amount of substance present.
Example: density is the same no matter how much substance is present

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30
Q

Chemical property

A

The ability or inability of a substance to combine with or change into one or more other substances
Example: rusting

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31
Q

Physical change

A

A change that alters a substance without changing its composition

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32
Q

Phase change

A

Transition of matter from one state to another

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33
Q

Chemical change

A

A process that involves one or more substances changing into new substances, commonly referred to as a chemical reaction

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34
Q

Law of conservation of mass

A

States that mass is neither created created nor destroyed during chemical reaction—it os conserved
Mass(reactants)=mass(products)

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35
Q

Mixture

A

A combination of two or more pure substances in which each pure substance retains its individual chemical properties.

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36
Q

Heterogeneous mixture

A

A mixture that does not blend smoothly throughout and in which the individual substances remain distinct

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37
Q

Homogeneous mixture

A

Mixture that has constant composition throughout; it always has a single phase

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38
Q

Solutions

A

A uniform mixture that can contain solids, liquids, or gases; also called a homogeneous mixture

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39
Q

Element

A

A pure substance that cannot be separated into simpler substances by physical or chemical means

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40
Q

Periodic table

A

Organizes the elements into a grid of horizontal rows called periods and vertical columns called groups or families

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41
Q

Compound

A

Pure substances made up of two or more different elements that are combined combined chemically

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42
Q

Democritus

A
  • matter is composed of atoms, which move through empty space.
  • atoms are solid, homogeneous, indestructible, and indivisible.
  • different kinds of atoms have different sizes and shapes.
  • size, shape, and movement of atoms determine the properties of matter
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43
Q

Aristotle

A
  • empty space cannot exist

- matter is made of earth, fire, air, and water

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44
Q

Dalton

A
  • matter is composed of extremely small particles called atoms
  • atoms are indivisible and indestructible
  • atoms of a given element are identical in size, mass, and chemical properties
  • atoms of a specific element are different from those of another element
  • different atoms combine in simple whole-number ratios to form compounds
  • in a chemical reaction, atoms are separated, combined or rearranged
45
Q

Law of Definite proportions

A

States that, regardless of the amount, a compound is always composed of the same elements in the same proportion by mass

46
Q

Law of Multiple Proportions

A

States that when different compounds are formed by the combination of the same elements, different masses of one element combine with the same fixed mass of the other element in a ratio of small whole numbers

47
Q

Atomic structure

A

At the centre of an atom is a nucleus containing protons and neutrons. Electrons are arranged around the nucleus in energy levels or shells

48
Q

Isotopes

A

Atoms with the same number of protons but different numbers of neutrons

49
Q

Mass number

A

The sum of the atomic number (or number of protons) and neutrons in the nucleus

50
Q

Isotope symbol

A

(mass number/atomic number)Chemical Symbol

51
Q

Atomic mass unit (amu)

A

One-twelfth the mass of a carbon-12 atom

52
Q

Radioactivity

A

The process in which some substances spontaneously emit radiation

53
Q

Radiation

A

The rays and particles emitted by the radioactive materials

54
Q

Nuclear reaction

A

A reaction that involves a change in an atom’s nucleus

55
Q

Radioactive decay

A

Unstable nuclei lose energy by emitting radiation in this spontaneous process

56
Q

Alpha radiation

A

The radiation that was deflected toward the negatively charged plate

57
Q

Alpha particle

A

Contains two protons and two neutrons, and thus has a 2+ charge, which explains why alpha particles are attracted to the negatively charged plate

58
Q

Nuclear equation

A

Equation that shows the atomic numbers and mass numbers of the particles involved

59
Q

Beta radiation

A

The radiation that was deflected toward the positively charged plate

60
Q

Beta particle

A

And electron with a 1- charge

61
Q

Gamma ray

A

A high-energy radiation that possesses no mass and is denoted by the symbol

62
Q

Beta decay

A

A radioisotope that lies above the band of stability is unstable because it has too many neutrons relative to its number of protons.

63
Q

Alpha decay

A

All nuclei with more than 82 protons are radioactive and decay spontaneously

64
Q

Electromagnetic radiation

A

A form of energy that exhibits wavelike behavior as it travels through space

65
Q

Nuclear power plant

A

In the chamber there are are control rods that control fission and absorb neutrons, and fuel rods with uranium in them. When the control rods are taken out, fission occurs which heats the water. The steam rises which heats a turbine that creates electricity through the generator. When the steam in the turbine cools it goes back to the chamber to be reheated

66
Q

Wavelength

A

The shortest distance between equivalent points on a continuous wave

67
Q

Frequency

A

The number of waves that pass a given point per second (Hz)

68
Q

Amplitude

A

The wave’s height from the origin to a crest, or from the origin to a trough

69
Q

Electromagnetic Wave Relationship

A

Speed of light in a vacuum (c)= (wavelength)(frequency)

70
Q

Relationship between wavelength and frequency

A

As wavelength increases, frequency decreases

71
Q

What happens when light passes through a prism?

A

It is separated into a continuous spectrum of its different components—red, orange, yellow, green, blue, indigo, and violet light

72
Q

Electromagnetic spectrum

A

Includes all forms of electromagnetic radiation; the types of radiation differ in their frequencies and wavelengths

73
Q

Bohr’s Model of the Atom

A

Depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus

74
Q

Ground state

A

The lowest allowable energy state of an atom

75
Q

Quantum number

A

The number assigned to each orbit of an electron

76
Q

Quantum

A

The minimum amount of energy that can be gained or lost by an atom

77
Q

Quantum mechanical model of the atom

A

An atomic model in which electrons are treated as waves; also called the wave mechanical model of the atom

78
Q

De Broglie Equation

A

Predicts that all moving particles have wave characteristics

79
Q

Particle Electromagnetic-Wave Relationship

A

Wavelength=Planck’s constant/(mass of the particle)(velocity)

80
Q

Heisenberg uncertainty principle

A

States that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time.

81
Q

Atomic orbital

A

Three-dimensional region around the nucleus which describes the electron’s probable location

82
Q

Energy sub levels

A

The energy levels contained within a principal energy level

83
Q

Shapes of orbitals

A
  • Sublevels are labeled s, p, d, or f according to the shapes of the atom’s orbitals
  • each orbital can contain, at most, two electrons
84
Q

Electron configuration

A

The arrangement of electrons in an atom

85
Q

Aufbau principle

A

States that each electron occupies the lowest energy orbital available

86
Q

Pauli exclusion principle

A

States that a maximum of two electrons can occupy a single atomic orbital, but only if the electrons have opposite spins

87
Q

Hund’s rule

A

States that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals

88
Q

Noble-gas notation

A

The electron configuration for an element can be represented using the noble-gas notation for the noble gas in the previous period and the electron configuration for the additional orbitals being filled

89
Q

Valence electrons

A

Electrons in the atom’s outermost orbitals—generally those orbitals associated with the atom’s highest principal energy level

90
Q

Periodic law

A

The statement that there is a periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number

91
Q

John Newlands

A
  • arranged elements by increasing atomic mass
  • noticed the repetition of properties every eighth element
  • created the law of octaves
92
Q

Lothar Meyer

A
  • demonstrated a connection between atomic mass and elements’ properties
  • arranged the elements in order of increasing atomic mass
93
Q

Dmitri Mendeleev

A
  • demonstrated a connection between atomic mass and elements’ properties
  • arranged the elements in order of increasing atomic mass
  • predicted the existence and properties of undiscovered elements
94
Q

Henry Moseley

A
  • discovered the atom contain a unique number of protons called the atomic number
  • arranged elements in order of increasing atomic number, which resulted in a periodic pattern of properties
95
Q

Groups

A

A vertical column of elements in the periodic table arranged in order of increasing atomic number; also called a family

96
Q

Periods

A

A horizontal row of elements in the modern periodic table

97
Q

Excited state

A

When an atom gains energy

98
Q

Atomic radius

A

The measure of the size of atoms. The distance from the atomic nucleus to the outermost electron orbital

99
Q

Ionization energy

A

The energy required to remove an electron from a gaseous atom

100
Q

Periodic trends

A

Atomic radius: decreases across and increases down

Ionization energy: increases across and decreases down

101
Q

Metals

A

Elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity

102
Q

Nonmetals

A

Elements that are generally gases or brittle, dull-looking solids

103
Q

Metalloids

A

Have physical and chemical properties of both metals and nonmetals

104
Q

Ion

A

An atom or a bonded group of atoms that has a positive or negative charge

105
Q

Chemical bond

A

The force that holds two atoms together

106
Q

Cation

A

Positively charged ions that forms when an atom loses one or more valence electrons in order to attain a noble gas configuration

107
Q

Anion

A

A negatively charged ion

108
Q

Inverse proportion

A

When one value increases the other value decreases

109
Q

Direct proportion

A

When one value increases the other value increases by the same percentage

H Chemisty I (5 decks)

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