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Chemistry 1 > Semester 1 Final > Flashcards

Semester 1 Final Flashcards

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0
Q

What is the chemical formula for ozone?

A

O3

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1
Q

What does the ozone layer do?

A

Protects living things on Earth from ultra violet waves

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2
Q

What are the two types of ozone?

A

Air-naturally occurs in the upper atmosphere (good)

Ground- created by exhaust and aerosol (large amounts are toxic)

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3
Q

How is ozone being depleted?

A

Chlorofluorocarbons (CFCs) and nitrous oxide

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4
Q

Independent variable

A

Value scientists plan on changing

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5
Q

Dependent variable

A

Value that changes in response to the change in the independent variable

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6
Q

Constant

A

Values that must stay the same throughout the experiment

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7
Q

Control

A

Standard used for comparison

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8
Q

Qualitative data

A

Information describing color, odor, shape, or some other physical characteristic (not able to be measured)

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9
Q

Quantitative data

A

Numerical information describe how much, little, big, tall, or fast (measurable Ex: height, length, volume)

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10
Q

Theory

A

Explanation of natural phenomenon based on many observations and investigations over time

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11
Q

Scientific law

A

Relationship in nature supported by many experiments

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12
Q

Difference between a theory and a law

A

There are no exceptions to laws; theories can be proved wrong

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13
Q

How do you calculate significant figures when multiplying/dividing?

A

Number of the least significant figures of the numbers being multiplied/divided= number of significant figures in answer
Ex:124.0 x 2.4= 297.6= 300

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14
Q

How do calculate significant figures when adding/subtracting?

A

Where the shortest number ends= where significant figure of product ends
Ex: 35.01 + 72.3+ 61= 168.31= 168

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15
Q

How to determine significant figures when measuring

A

Sig figs go to the closest measuring mark, then a guess

Ex: measuring cm: 55.40

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16
Q

Chemical change

A

Change that involves one or more substances changing into new substances
Ex: burning, reaction, neutralization

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17
Q

Physical change

A

Change that alters a sample without changing its composition

Ex: tearing, grinding, mixing

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18
Q

Accuracy

A

How close a measured value is to the accepted value (right answer)

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19
Q

Precision

A

How close a series of measurements are to eachother rather than the accepted value (May be wrong, but consistently wrong)

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20
Q

Density

A

Amount of mass per unit of volume

D= m/v

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21
Q

Label for density?

A

G/cm cubed or g/mL

(1cm cubed= 1 mL

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22
Q

Slope formula?

A

x2-x1

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23
Q

Between what numbers must the coefficient be in scientific notation?

A

1 and 10

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24
Q

What is the exponent when you move the decimal to the right?

A

Negative

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25
Q

What is the exponent when you move the exponent to the left?

A

Positive

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26
Q

Mixture

A

Combination of 2 or more pure substances in which each pure substance retains its individual chemical properties

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27
Q

Two kinds of mixtures?

A

Heterogeneous and homogeneous

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28
Q

Heterogeneous mixture

A

Mixture that doesn’t blend smoothly throughout and individual substances remain distinct
Ex: chez mix, pepperoni pizza

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29
Q

Homogeneous mixture

A

Mixture that has a constant composition throughout (also called solution)
Ex: black coffee, salt water

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30
Q

Intensive properties

A

Property that remains the same no matter how much of the substance is present
Ex: density, color, flammability, solubility

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31
Q

Extensive properties

A

Property that is dependent upon the amount of substance present
Ex: length, mass, volume

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32
Q

States of matter

A

Physical forms in which all matter exists on earth (physical property)

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33
Q

Name the three states of matter

A

Solid, liquid, gas

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34
Q

Solid

A

Has its own definite shape and volume, is incompressible, and expands only slightly when heated
Ex: ice

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35
Q

Liquid

A

Flows, has constant volume, and takes the shape of the container
Ex: water

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36
Q

Gas

A

Flows to conform to shape of container, fills containers entire volume, and is easily compressed
Ex: water vapor

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37
Q

Compound

A

Made up of two or more different elements that are combined chemically
-type of pure substance
Ex: salt, water, sugar

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38
Q

What four things are shown in a box on the periodic table?

A
  • atomic number
  • chemical symbol
  • name of element
  • mass number(AVG mass of all known isotopes)
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39
Q

Contribution to the Atomic Theory: Chadwick

A

Discovered the neutron

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40
Q

Contribution to the Atomic Theory: Thompson

A

Discovered the electron and charge to mass ratio (plum pudding model)

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41
Q

Contribution to the Atomic Theory: Rutherford

A

Discovered atoms were mostly empty space, which led him to discover the proton and nucleus

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42
Q

Contribution to the Atomic Theory: Bohr

A

Created quantum model for the hydrogen atom to explain its atomic emission spectrum
Created ground state (lowest energy level) as well as quantum numbers.
-models flaw: didn’t explain AES for any other element

43
Q

Electron

A

Negatively charged subatomic particles

-located outside nucleus

44
Q

Nucleus

A

Small, densely packed center of an atom; made of protons of neutrons

45
Q

Protons

A

Positively charged subatomic particles

  • located in nucleus
  • mass: 1amu
46
Q

Neutron

A

Subatomic particle with no charge

  • located in nucleus
  • mass: 1amu
47
Q

How to find mass number of an element?

A
  • Multiply the mass of each isotope by its occurrence percentage
  • add the product of each isotope to find the final mass number
48
Q

What does the isotope symbol tell you?

A

Element and symbol, atomic mass (top left), and atomic number (bottom left)

49
Q

Crest

A

Highest point on a wave

50
Q

Trough

A

Lowest point on a wave

51
Q

Wavelength

A

Shortest distance between equivalent points on a continuous wave (crest to crest, trough to trough)

52
Q

Amplitude

A

Waves height from origin to crest/trough

53
Q

Frequency

A

Number of waves that pass a given pint per second

  • symbol: v
  • measured in hertz (Hz)
54
Q

Longer wavelength=???

A

Lower frequency

Like a spring

55
Q

Short wavelength=???

A

Higher frequency

Like a spring

56
Q

Electromagnetic radiation

A

Form of energy that exhibits wavelike behavior as it travels through space

57
Q

Electromagnetic spectrum (EM spectrum)

A

Includes all forms of electromagnetic radiation with only difference in types of radiation being in wavelength and frequency

58
Q

Types of EM radiation (7)

Lowest to highest frequency/ highest to lower wavelength

A 
Radio
Microwave
Infrared
Visible light (red: lowest frequency violet: highest frequency)
UV
X-rays 
Gamma rays
59
Q

Valence electron

A

Electrons in the outermost energy levels

60
Q

What do valence electrons determine?

A

Bonding, reaction, and oxidation number

61
Q

Valence electrons in each group

A 
Group 1(Alkali metal): 1
Group 2(alkaline earth metals): 2
Group 3-12: multi alert except for Cd, Ag, and Zn
Group 13(boron group): 3
Group 14(Carbon group): 4
Group 15(nitrogen group): 5
Group 16(chlacogens): 6
Group 17(Halogens): 7
Group 18(Noble gases): 8 (except He: 2)
62
Q

Electron dot structure

A

Element symbol plus dots signifying number of valence electrons

63
Q

Oxidation number

A

Positive/negative charge of an atom as a result of forming an ion

64
Q

What groups form positive ions(cation)?

A

Any group with less than 4 valence electrons

Group 1-13

65
Q

What groups form negative ions(anion)?

A

Groups 15-17

66
Q

What is the oxidation number for the carbon group?

A

Positive or negative 4 (depends what it’s being bonded with)

67
Q

Why don’t noble gases have oxidation numbers?

A

Huey have a full set of outer level electrons, so they don’t react with any other element

68
Q

Oxidation numbers of each group

A

1: +1
2: +2
3-12: multivalent
13: +3
14: - or + 4
15: -3
16: -2
17: -1

69
Q

What transition metals have fixed charges?

A

Silver (Ag): +1

Cadmium (Cd) and zinc (Zn): +2

70
Q

Electron configuration

A

Arrangement of electrons in an atom

71
Q

Aufbaus rule

A

Each electron occupies the lowest energy orbital available

72
Q

Paulis exclusion principle

A

A max of 2 electrons can occupy a single atomic orbital but only of the electrons have opposites spins

73
Q

Hunds rule (bus rule)

A

Single electrons with he same spins must occupy each energy level before additional electrons with opposite spins can occupy the same orbital
(Each one gets 1 before any get 2)

74
Q

Sub levels: orbitals and max electrons

A

S: 1 orbital; holds up to 2 electrons
P: 3 orbitals; holds up to 6 electrons
D: 5 orbitals; holds up to 10 electrons
F: 7 orbitals; holds up to 14 electrons

75
Q

What groups do each sub level make up?

A

S- group 1 and 2 plus Helium
P- 13-18 except helium
D- 3-12
F- lanthanides and actinides

76
Q

Noble gas configuration

A

Last noble gas in brackets then he rest of the configuration

Ex: aluminum- [Ne]3s23p1

77
Q

Orbital diagrams

A

Represents each electron in every orbital/sub level

  • arrows must point opposite ways (Pauli)
  • lowest level must be filled before moving on (Aufbau)
  • each one must get 1 before any get 2 (Hund)
78
Q

Groups

A

Columns

79
Q

Periods

A

Rows

80
Q

Ionization energy

A

Energy required to remove an electron from an atom

Decreases down group, increases across period

81
Q

Atomic radius

A

Distance across an atom

Increases down group decreases across period

82
Q

Electron negativity

A

Relative ability of an atom to attract electrons

Decreases down group, increases across period

83
Q

Characteristics of metals (5)

A

Good conductors, malleable, ductile, high melting and boiling points, shiny

84
Q

Characteristics of no metals (5)

A

Generally gases, dull, brittle, poor conductors, low melting and boiling points

85
Q

Characteristics of metallics

A

Characteristics of both metals and nonmetals

86
Q

What did Dmitri Mendeleev contribute to the periodic table?

A

Arranged elements in increasing atomic mass

-left room for undiscovered elements and actually predicted some of their properties

87
Q

What did Henry Mosley contribute to the periodic table?

A

Discovered relationship between atomic number and number of protons and arranged elements by increasing atomic number

88
Q

Alpha particle

A

Particle with two protons and two neutrons, with and +2; equivalent to a helium-4 nucleus and is emitted by radioactive decay

89
Q

Alpha radiation

A

Radiation made up of alpha particles; deflected towards negatively charged plate when directed between two electrically charged plates
-blocked with sheet of paper

90
Q

Beta particle

A

High speed electron emitted during radioactive decay

91
Q

Beta radiation

A

Radiation made up of beta particles; deflected toward positively charged plate when directed between two electrically charged plates
(Moves more than alpha radiation because it has less mass)
-blocked with sheet of lead

92
Q

Gamma ray

A

High energy radiation with no mass and no charge; not deflected toward either plate and usually accompanies alpha and beta radiation

  • accounts for most energy lost during radioactive decay
  • blocked by block of lead
93
Q

Where does the radiation go in a decay equation?

A

Product side (right)

94
Q

Where does radiation go in a capture equation?

A

Reactant side (left)

95
Q

Chemical bond

A

Force that holds two atoms together

96
Q

Two types of chemical bonds

A

Covalent and ionic

97
Q

Covalent bond

A

Formed by the sharing of electrons (between two non metals)

98
Q

Ionic bond

A

Formed by the transfer of electrons (between cation and anion/ metal and nonmetal)

99
Q

How to name a binary ionic compound

A

Metal then nonmetal with -IDE ending; CHARGES MUST MATCH!

Ex: magnesium sulfide: MgS

100
Q

How to name multivalent ionic compounds

A

Metal (Roman numeral) then nonmetal with -IDE ending; CHARGES MUST MATCH!
Any metal 3-12 have multiple oxidation numbers indicated by Roman numeral
Ex: copper (I) sulfide: Cu2S

101
Q

How to name polyatomic ionic compounds

A

Metal (and Roman numeral if needed) then polyatomic ion. CHARGES MUST MATCH! Parentheses if adding subscript to polyatomic
-all polyatomic ions are negative except ammonium (NH4)
Ex: aluminum nitrate: Al(NO3)3

102
Q

How to name molecular compounds

A

Covalent: first nonmetal with prefix (unless subscript is one) then second nonmetal with prefix
Ex: disulfur pentoxide: S2O5

103
Q

How to name hydrates

A

Hydrate: compound containing water
Normal ionic name + H2O with a prefix
Ex: aluminum nitrate octahydrate: Al(NO3)3:8H2O
:= dot

104
Q

Naming rules for acids (3)

A 
MUST HAVE HYDROGEN FIRST!
end in -ide: hydro\_\_\_\_\_\_\_ic acid
Ex: HBr: hydrobromic acid (charges must match)
end in -ate: \_\_\_\_\_\_ic acid
Ex: H2SO4: sulfuric acid
end in -ite: \_\_\_\_\_\_ous acid
Ex: HClO2: chlorous acid

Chemistry 1 (5 decks)

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