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Bio lab test > Chem Ch 1 > Flashcards

Chem Ch 1 Flashcards

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1
Q

Empirical

A

Based on observation and experiment

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2
Q

Qualitative

A

Noting or describing how a process happens

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3
Q

Quantitative

A

Measuring or quantifying how something happens

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4
Q

Hypothesis

A

Tentative interpretation or explanation of the observation

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5
Q

Falsifiable

A

A good hypothesis is falsifiable, meaning it makes predictions that can be confirmed or refuted by further observations

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6
Q

Experiments

A

Highly controlled procedures designed to generate observations that can confirm or refute a hypothesis

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7
Q

Scientific Law

A

A brief statement that summarizes past observations and predicts new ones.

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8
Q

Law of Conservation of Mass

A

In a chemical reaction, matter is neither created or destroyed.

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9
Q

Scientific Theory

A

A model for the way nature is; tries to explain not merely what nature does, but why. Made of one or more well-established hypotheses.

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10
Q

Atomic theory

A

Proposed by John Dalton. each element is composed of tiny, indestructible particles called atoms. All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements. Atoms combine in simple, whole number ratios to form compounds. Atoms of one element cannot change into atoms of another element. In a chemical reaction, atoms change the way they are bound together with other atoms to form a new substance.

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11
Q

Matter

A

Anything that occupies space and has mass. It is classified according to its state (solid, liquid, gas)

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12
Q

Substance

A

A specific instance of matter (air, water, sand)

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13
Q

Solid matter

A

Atoms are packed closely together in fixed locations. The atoms vibrate, but do not move around each other. Has fixed volume and rigid shape. May be crystalline or amorphous.

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14
Q

Crystalline

A

Solid matter with atoms arranged in patterns with long-range, repeating order (table salt, diamond).

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15
Q

Amorphous

A

Solid matter without any long-range order to its atoms or molecules (glass, plastic).

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16
Q

Liquid Matter

A

Atoms pack as closely as they do in a solid, but they move around and assume the shape of their container.

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17
Q

Gaseous Matter

A

Atoms and molecules have a lot of space between them and are free to move relative to one another, making gases compressible and fluid.

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18
Q

Composistion

A

The kinds and amounts of substances that compose a substance.

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19
Q

Classification of matter order:

A

Matter
Pure substance or Mixture
Pure substances - elements or compounds?
Mixtures - Heterogeneous or homogeneous?

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20
Q

Element

A

Substance that cannot be chemically broken down into simpler substances.

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21
Q

Compound

A

Substance composed of two or more elements in fixed, definite proportions. More common than elements.

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22
Q

Heterogeneous mixture

A

Composition varies from one region to another

23
Q

Homogeneous mixture

A

Composition is the same throughout

24
Q

Physical changes

A

Changes that only alter state or appearance, but not composition. The atoms or molecules that compose their substance do not change their identity during a physical change (boiling water).

25
Q

Chemical changes

A

During a chemical change, atoms rearrange, transforming the original substances into different substances (rusting iron).

26
Q

Physical property

A

A property that a substance displays without changing its composition of character (smell).

27
Q

Chemical property

A

A property that a substance displays only by changing its composition via a chemical change (flammability, acidity, toxicity, corrosiveness).

28
Q

Energy

A

The capacity to do work

29
Q

Work

A

The action of a force through a distance

30
Q

Kinetic energy

A

Energy associated with its motion.

31
Q

Potential

A

Energy associated with an objects position or composition.

32
Q

Total energy

A

The sum of kinetic and potential energies.

33
Q

Thermal energy

A

The energy associated with the temperature of an object. Actually a type of kinetic energy because it arises from the motion of the individual atoms or molecules that make up an object. Example: weight hits the ground, kinetic energy is transferred to the atoms of the ground, raising ground’s temperature.

34
Q

Law of conservation of energy

A

Energy is neither created or destroyed.

35
Q

Second principle about change of energy

A

Systems with high potential energy tend to change in ways that lower their potential energy.

36
Q

Unstable objects

A

Systems with high potential energy

37
Q

SI base units

A

Meter, kilogram, second, Kelvin, Mole, Ampere, Candela

38
Q

Kilogram measures what?

A

Mass, different from weight.

39
Q

Mass

A

A measure of the quantity of matter within an object

40
Q

Weight

A

The gravitational pull on matter within an object.

41
Q

Example of difference between mass and weight.

A

Weight on moon changes because of a weaker gravitational pull, mass stays the same.

42
Q

Kelvin

A

Avoids negative temperatures. 0 K = -273 C (absolute zero).

43
Q

Kelvin to celsius conversion

A

K = C + 273.15

44
Q

Name all the prefixes, their symbols, and their multipliers.

A 
exa, E, 10^18
peta, P, 10^15
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, weird u, 10^-6
nano, n, 10^-9
pico, p, 10^-12
femto, f, 10^-15
atto, a, 10^-18
45
Q

Derived unit

A

A combination of other units (meters per second).

46
Q

Volume

A

Measure of space. Unit of length cubed.

47
Q

Density

A

Ratio of mass to volume, d = m/v

48
Q

Intensive property

A

Property that is independent of the amount of substance there is (density).

49
Q

Extensive property

A

Property that depends on the amount of substance (mass, weight).

50
Q

Uncertainty of sigfigs

A

Reported in the last digit. Assumed to be + or - 1 of the last digit. Last digit is estimated.

51
Q

Exact numbers

A

Have no uncertainty. Do not limit the number of sigfigs. Can originate from accurate counting of discrete objects or defined quantities, like the number of centimeters in 1 m. Also from integral numbers, numbers that are part of an equation (diameter/2).

52
Q

Accuracy

A

Refers to how close the measured value is to the actual value.

53
Q

Precision

A

Refers to how close a series of measurements are to one another or how reproducible they are.

54
Q

Dimensional analysis

A

Using units as a guide to problem solving

Bio lab test (3 decks)

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