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Chemistry > Test 1 > Flashcards

Test 1 Flashcards

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1
Q

Why study chemistry?

A

It helps to explain why things are the way they are.

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2
Q

Where are chemicals?

A

Everywhere.

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3
Q

Define matter (ON TEST)

A

Anything that has mass and occupies space.

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4
Q

Define chemistry

A

The study of the composition, structures, and properties of matter and the reactions they undergo.

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5
Q

What is matter made of?

A

Elements

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6
Q

What makes up compounds?

A

Elements

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7
Q

What are the five branches of chemistry?

A

Organic - the study of carbon-containing substances
Inorganic - the study of non-carbon-containing substances that are bonded to metals
Physical - the study of the properties and changes of matter and their energy relationships
Nuclear - the study of radiation
Biochemistry - the study of living things (Peter Parker does this!)

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8
Q

What are the two types of research?

A

Basic (designed to increase knowledge) and applied (designed to solve a problem)

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9
Q

Name the steps of the scientific method

A
  1. Observation
  2. Hypothesis
  3. Experimentation (proceed to step 4 or go back to 2)
  4. Theory
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10
Q

Define scientific method

A

A systematic way of observing, experimenting, and solving problems

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11
Q

Define significant figures

A

Measured numbers that are reliable and accurate. Numbers that are measured so that every digit is certain, except the last which is estimated

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12
Q

Name 6 rules for significant figures (ON TEST)

A
  1. All nonzero numbers are significant
  2. Exact numbers have infinite significance
  3. Zeros trailing nonzero numbers are not significant (Ex; 80, 7700, 9990000)
  4. Leading zeros are not significant (Ex; 0.1, 0.0045)
  5. Zeros trapped between nonzero numbers are significant (Ex; 4033, 2001)
  6. Zeros trailing a nonzero number, and a decimal being present, are significant (Ex; 1.00, 20.00)
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13
Q

Multiply and dividing sig figs rule

A

The answer carries the same number of sig figs as the factor with the fewest sig figs.
Example: 12.04*5.4=65.016=65

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14
Q

Adding and subracting sig figs

A

The answer carries the same number of decimal places as the factor carrying the fewest decimal places.
Example: 63.4+0.16=63.56=63.6

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15
Q

Rounding numbers rule

A

If the last number is exactly 5, and the number preceding it is even, it rounds to the even number. However, if the number preceding it was odd, then it will round up to the next number.
Example: 3.45=3.4 or 3.55=3.6

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16
Q

What are the basic units of measurement?

A

Length - meters
Mass - kilograms (official) or grams (base)
Temperature - Kelvin
Time - seconds

17
Q

The base units of the metric system?

A

Meters, grams, liters, seconds, joules, calories

18
Q

The metric system prefixes, symbols, and multipliers?

A

Tera - T - 10^12
Giga - G - 10^9
Mega - M - 10^6
Kilo - k - 10^3
Deci - d - 10^-1
Centi - c - 10^-2
Milli - m - 10^-3
Micro - µ - 10^-6
Nano - n - 10^-9
Pico - p - 10^-12
Femto - f - 10^-15

19
Q

Define volume

A

A measure of space

20
Q

Step for converting units of measurement

A
  1. Identify the given term
  2. Identify what term is to be found
  3. Multiply the given conversion factor so that the unit of the given term is canceled out
  4. Check your answer
21
Q

Define density

A

The amount of mass per unit volume

22
Q

What are the measurements of density for solids, liquids, and gases

A

Solids - g/cm^3
Liquids - g/mL
Gases - g/L

23
Q

The formulas for mass, density, and volume

A

Density = mass/volume
Mass = density*volume
Volume = mass/density

24
Q

Give identifying traits of a solid

A

-Definite shape
-Definite volume
-Incompressible
–Amorphous (unspecific bonds)
–Crystalline (specificity in bonds)

25
Q

Give identifying traits of a liquid

A

-Indefinite shape
-Definite volume
-Incompressible

26
Q

Give identifying traits of a gas

A

-Indefinite shape
-Indefinite volume
-Compressible

27
Q

What are the classifications of matter? (ON TEST)

A

Pure Substances
-Elements
-Compounds
Mixtures
-Homogenous (is consistent and distributed evenly throughout)
-Heterogenous (is inconsistent and is not distributed evenly throughout)

28
Q

Name the Identifications of Matter (ON TEST) (Hint: there are 4)

A
  1. Physical properties
    -Characteristics of a substance that can be observed w/o changing the substance
  2. Chemical properties
    -The reactions that substances undergo
  3. Physical changes
    -A change of state that a substance undergoes (Ex: water melting, evaporating, sublimating, freezing, condensing, or depositing)
  4. Chemical changes
    -A change in the composition or arrangement of atoms in a compound resulting in a new form of substance
29
Q

Name the three ways of separating mixtures and where they apply (ON TEST)

A
  1. Decanting
    -When moving a liquid away from a solid
  2. Distillation
    -When moving two liquids away from each other
    -“With a mixture of liquids, one may be more volatile and by heating the distillation apparatus, the liquids can be separated.”
  3. Filtration
    -When moving two solids away from each other (using a liquid as a dissolver)
30
Q

State the law of the conservation of mass

A

Matter can be neither created nor destroyed in a chemical reaction. (Nuclear reaction exempt)

31
Q

State the law of the conservation of energy

A

Energy can be neither created nor destroyed. (Nuclear reaction exempt)

32
Q

Name the four types of energy

A
  1. Kinetic energy
  2. Potential/stored energy
  3. Electric energy
  4. Chemical energy
33
Q

What units of measurement are used for energy?

A

Joules and calories

34
Q

What are the three temperature scales?

A
  1. Fahrenheit
    -(32)° is the freezing point for water, and 212° is the boiling point of water. Effective between -40° and 650°, which are the freezing and boiling points of mercury, respectively.
  2. Celsius
    -0° is the freezing point of water, and 100° is the boiling point.
  3. Kelvin
    -0°K is when all matter stops moving. 273.15° is the freezing point of water, and 373.15° is the boiling point.
35
Q

Temperature conversion formulas (ON TEST)

A

F to C - °C = (x°F - 32)(5/9)
C to F - °F = (x°C)(9/5)+32
C to K - K = °C + 273.15
K to C - C = K - 273.15

36
Q

Define heat capacity

A

The quantity of heat energy required to change the temperature of a given amount of the substance by 1°C

37
Q

Define specific heat

A

The heat capacity of a substance for 1g of the substance. Measured in J/g°C

38
Q

Give the formula for heat

A

q = mCΔT
q means heat
m means mass
C means specific heat
ΔT means the change in heat/temperature

39
Q

Scientific Notation

A

Scientific notation is a way of writing very large or very small numbers. A number is written in scientific notation when a number between 1 and 10 is multiplied by a power of 10. For example, 650,000,000 can be written in scientific notation as 6.5 ✕ 10^8.

Chemistry (3 decks)

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