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General Chemistry > Terms > Flashcards

Terms Flashcards

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0
Q

Quantitative Information

A

Numerical data

Example: temperature at which a chemical substance melts or has mass

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1
Q

Hypothesis

A

A tentative explanation/prediction based on experimental observations.

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2
Q

Qualitative Information

A

Consists of non numerical observations

Example: color of substance/physical appearance

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3
Q

Law

A

A concise verbal/mathematical statement of a behavior/relation that seems always to be the same under the same conditions.

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4
Q

Theory

A

A well tested, unifying, principle that explains a body of facts and the laws based on them; based on carefully determined and reproducible evidence.

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5
Q

State

A

An easily observed property (solid, liquid, or gas)

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6
Q

Kinetic-molecular theory of matter

A

All matter consists of extremely tiny particles (atoms, molecules, or ions) that are in constant motion.

In solids these particles are packed closely together, usually in a regular array. The particles vibrate back and forth about their average positions, but seldom do particles in a solid squeeze past their immediate neighbors to come into contact with a new set of particles.

The particles in liquids are arranged randomly rather than in the regular patterns found in solids. Liquids and gases are fluid because the particles are not confined to specific locations and can move past one another.

Under normal conditions, the particles in a gas are far apart. Gas molecules move extremely rapidly and are not constrained by their neighbors. The volume of a gas sample is the volume of he container in which it is held.

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7
Q

Kinetic energy

A

The energy of motion of the particles

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8
Q

Macroscopic

A

Visible to the naked eye

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9
Q

Submicroscopic/particulate world

A

Made up of individual particles that make up all matter

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10
Q

Solution

A

A homogeneous mixture of water and dissolved substances (liquid state)

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11
Q

Homogenous Mixture

A

A mixture which consists of 2 or more substances in the same phase. (A solution)

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12
Q

Heterogenous Mixture

A

A mixture in which the uneven texture of the material can be detected.

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13
Q

Purified Substance

A

When mixture which has been separated into its pure components

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14
Q

Elements

A

Substances that are composed of only one type of atom

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15
Q

Periodic Table

A

A table in which the symbol and other information for the elements are closed in a box.

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16
Q

Atom

A

The smallest particle of an element that retains the characteristic chemical properties of that element.

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17
Q

Chemical Bonds

A

Something that holds elements together

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18
Q

Chemical compound

A

A pure substance which is composed of two or more different elements

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19
Q

Ions

A

Electrically charged atoms or groups of atoms

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20
Q

Molecules

A

The smallest discrete units that retain the composition and chemical characteristics of the compound

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21
Q

Chemical formula

A

This represents the composition of any compound.

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22
Q

Physical properties

A

Properties which can be observed and measured without changing the composition of a substance.

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23
Q

Density

A

The ratio of the mass of an object to its volume which is a physical property useful for identifying substances.

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24
Q

Teperature

A

This often affects the numerical values of a property.

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25
Q

Extensive properties

A

These depend on the amount of a substance present

26
Q

Intensive properties

A

These font depend on the amount of substance

27
Q

Physical changes

A

Changes in physical properties; in this type of change the identity of a substance is preserved even though it may have changed its physical state or the gross size and shape of its pieces

28
Q

Chemical change

A

A reaction in which one or more substances (reactants) are transformed into one/more different substances (products)

29
Q

Chemical equation

A

The representation of the change using chemical formulas; it shows that the reactants (on left side of equation) produce the substances on the right (products)

30
Q

Chemical property

A

This indicates whether and sometimes how readily a material undergoes a chemical change with another material.

31
Q

Thermal energy

A

The motion of atoms, molecules, or ions at the submicroscopic (particulate) level (thermal energy.) All matter has thermal energy. (A form of kinetic energy.)

32
Q

Mechanical energy

A

The motion of macroscopic objects such as a moving tennis ball or automobile. (A form of kinetic energy.)

33
Q

Electrical energy

A

Movement of electrons in a conductor. (A form of kinetic energy.)

34
Q

Acoustic energy

A

The compression and expansion of the spaces between molecules in the transmission of sound. (A form of kinetic energy.)

35
Q

Gravitational energy

A

Energy possessed by a ball held above the floor and by water at the top of a water wheel. (Potential energy)

36
Q

Chemical energy

A

Potential energy stored in fuels; almost all chemical reactions involve a change in chemical energy

37
Q

Electrostatic energy

A

Potential energy associated with the separation of two electrical charges.

38
Q

Law of conservation of energy

A

Energy can neither be created nor destroyed; the total energy can neither be created nor destroyed; the total energy of the universe is constant.

39
Q

Metric system

A

A decimal system used internationally in science

40
Q

SI

A

The Système International d’Unités (international system of units); these units are derived from base units.

41
Q

Absolute zero

A

The lowest temperature that can be achieved.

42
Q

Precision

A

This indicates how well several determinations of the same quantity agree.

43
Q

Accuracy

A

The agreement of a measurement with the accepted value of the quantity.

44
Q

Error in measurement = ?

A

Experimentally determined value - accepted value

45
Q

Percent error = ?

A

[(Error in measurement) / (accepted value)] x 100%

46
Q

Standard deviation

A

This is equal to the square root of the sum of the squares of the deviations for each measurement from the average, divided by one less than the # of measurements.

  1. Calculate avg. of measurements
  2. Determine the difference between measurement and average
  3. Square the results of step 2
  4. Add results of step 3
  5. Divide the sum of step 4 by the number of determinations minus 1
  6. Take the square root of the result
47
Q

Fixed notation

A

A fixed number

48
Q

Exponential/Scientific Notation

A

A way of presenting very large/small numbers in a compact and consistent form that simplifies calculations.

A x 10^b

49
Q

Significant figures

A

The digits in a measured quantity that were observed with the measuring device

50
Q

Dimensional Analysis

A

A general problem-solving approach that use the dimensions/units of each value to guide us through calculations.

51
Q

Conversion factor

A

An equation which expresses the equivalence of a measurement in two different units.

52
Q

Atomic number

A

The number of protons in the nucleus of an element.

Z is the symbol which indicates the atomic number.

53
Q

Atomic mass unit (amu/u)

A

One amu is one-twelfth of the mass of an atom of carbon with 6 neutrons. (1 amu = 1.661x10^-24 g)

54
Q

Mass number

A

The sum of the number of protons & neutrons for an atom.

Number of protons + number of neutrons = mass number

55
Q

Isotopes

A

Atoms with the same atomic number but different mass numbers. (Always have some number of protons.)

56
Q

Atomic weight

A

The average mass of a representative sample of boron atoms

57
Q

Periodicity

A

Periodic repetition of the properties of elements; if the elements are arranged in order of increasing atomic mass, elements with similar properties appeared in a regular pattern.

58
Q

Law of chemical periodicity

A

The properties of the elements are periodic functions of atomic number.

59
Q

Groups/families

A

Elements that are arranged so that those with similar chemical and physical properties lie in vertical columns.

60
Q

The A groups

A

Main group elements

61
Q

The B groups

A

Transition elements

62
Q

Periods

A

Horizontal rows of the table

General Chemistry (4 decks)

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