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Honors Chemistry > Unit 2 > Flashcards

Unit 2 Flashcards

Introduction to Chemistry

1
Q

Chemistry

A

the study of the composition, structure, and properties of matter, the process that matter undergoes, and the energy changes that accompany these processes.

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2
Q

Matter

A

the material substance that forms the observable universe.

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3
Q

Mass

A

the measure of the amount of matter an object contains disregarding the shape of the object.

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4
Q

Atom

A

the smallest unit of an element that maintains the chemical identity of a specific element. This is known as the “building block of matter.”

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5
Q

Element

A

a pure substance that cannot be broken down into simpler, stable substances and is made of one type of atom.

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6
Q

Compound

A

a substance that can be broken down into simpler stabler substances. Each compound is made from the atoms of two or more different elements that are chemically bonded together.
ex. carbon dioxide, water

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7
Q

Molecule

A

the smallest unit of a compound that retains all the properties of that compound.

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8
Q

Extensive Property

A

Properties that depend on the amount of matter that is present.
ex. Volume, Mass, Energy Concentration

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9
Q

Intensive Property

A

Properties that do not depend on the amount of matter that is present.
ex. Melting Point, Boiling Point, Density, Ability to Conduct Electricity

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10
Q

Physical Property

A

A characteristic that can be observed or measured without changing the identity of the substance. Physical properties describe the substance itself, rather than describing how it can change into other substances.
ex. Water has a tendency to transition from a liquid to a solid when at 0oC. (i.e. Freezing Point)

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11
Q

Physical Change

A

A change in a substance that does not involve a change in the identity of the substance. These changes are usually reversible
ex. Grinding, Cutting, Melting, Boiling

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12
Q

Chemical Property

A

A substance’s ability to undergo changes that transform it into different substances. Chemical properties are easiest to see when substances react to form new substances.
ex. Carbon being able to burn in air.

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13
Q

Chemical Change

A

A change in which one or more substances are converted into different substances. These changes are usually irreversible
ex. Cooking, Rusting, Rotting

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14
Q

Solid

A

Matter that has a definite shape AND definite volume.

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15
Q

Liquid

A

Matter that doesn’t have a definite shape but has a definite volume.

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16
Q

Gas

A

Matter that doesn’t have a definite shape nor a definite volume.

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17
Q

Pure Substance

A

A classification of matter in which the composition of a substance is the same throughout and does not vary from sample to sample. A pure substance can be an element or a compound.

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18
Q

Mixture

A

A classification of matter in which there is a blend of two or more kinds of matter, each of which retains its own identity and properties.

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19
Q

Homogeneous Mixture

A

A substance that is uniform in composition.
ex. air, window cleaner, stainless steel

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20
Q

Heterogeneous Mixture

A

A substance that is not uniform in composition.
ex. granite, wood, blood

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21
Q

Periodic Table

A

a tabular array of the chemical elements organized by atomic number, from the element with the lowest atomic number (1), Hydrogen, to the element with the highest atomic number (118), Oganesson.

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22
Q

Periodic Law

A

If you arrange elements by atomic number (originally thought atomic mass), they will fall into recurring groups, so the elements with similar properties will appear in regular intervals.

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23
Q

Group

A

the vertical columns of the Periodic Table. Elements within groups have similar chemical properties, but have very different atomic structures.

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24
Q

Period

A

the horizontal rows of the Periodic Table.
Elements across a period have very different chemical properties, but share similar atomic structure.

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25
Q

Atomic Symbol

A

a element that is represented by a letter or letters.

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26
Q

Family

A

particular selection of elements in which all share relatively similar physical properties.

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27
Q

Luster

A

The ability of something to ‘shine’ based off its reflective surface.

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28
Q

Malleable

A

The ability not breaking or cracking after being hammered or bended.

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29
Q

Ductile

A

The ability to be stretched into a thin wire (similar to malleability).

30
Q

Group 1 – Alkali Metals

A

Very reactive, soft, low Melting/Boiling Point, not very dense.

31
Q

Group 2 – Alkaline Earth Metals

A

Slightly less reactive, but harder/denser compared to Alkali Metals.

32
Q

Group 3-12 – Transition Metals

A

Shiny, high Melting/Boiling Points, very dense, strong, good conductors.

33
Q

Assorted Groups – Post Transition Metals

A

Shiny, high Melting/Boiling Points (lower than Transition); more brittle.

34
Q

Hidden in 3 – Lanthanides

A

Shiny silvery-white metals that tarnish when exposed to air. Magnetic.

35
Q

Hidden in 3 – Actinides

A

Silverish in color metals that are radioactive. Tarnish readily in air.

36
Q

Assorted Groups – Metalloids // Semiconductors

A

Have properties of both metals and nonmetals (sometimes referred to as semiconductors or semimetals). Not as malleable compared to metals, but more malleable compared to nonmetals. Solid at room temperature.

37
Q

Assorted Groups – Other Non Metals

A

Poor conductors of heat and electricity. Either solid or gas at room temperature (besides Br). Brittle.

38
Q

Group 17 - Halogens

A

Nonmetals that are very reactive. Inflammable, but conduct electricity.

39
Q

Group 18 - Nobel Gasses

A

Unreactive, very stable. Gasses at room temperature.

40
Q

Melting

A

when a solid form of a substance transitions to a liquid form.

41
Q

Freezing

A

when a liquid form of a substance transitions to a solid form.

42
Q

Vaporization

A

when a liquid form of a substance transitions to a gaseous form.

43
Q

Condensation

A

when a gaseous form of a substance transitions to a liquid form.

44
Q

Deposition

A

when a gaseous form of a substance directly transitions to a solid form with no liquid intermediate.

45
Q

Sublimation

A

when a solid form of a substance directly transitions to a gaseous form with no liquid intermediate.

46
Q

Melting Point

A

the temperature needed for a specific substance to transition from a solid to liquid.

47
Q

Freezing Point

A

the temperature needed for a specific substance to transition from a liquid to solid.

48
Q

Boiling Point

A

the temperature needed for a specific substance to transition from a liquid to gas.

49
Q

Condensing Point

A

the temperature needed for a specific substance to transition from a gas to liquid.

50
Q

Hardness

A

the ability to resist being indented, deformed, or abraded because of its strength.
ex. a fingernail can scratch Gypsum, but Calcite would scratch a fingernail.

51
Q

Malleability

A

the ability to be hammered or pressed permanently out of shape without breaking or cracking.

52
Q

Rockwell and Brinell Test

A

The object’s malleability can be measured by checking the depth of indentation of a substance (Rockwell) and the width of an indentation of a substance (Brinell).

53
Q

Solubility

A

the maximum amount of solute that will dissolve in a given amount of solvent at a certain temperature.

54
Q

Solute

A

substance that is being dissolved.

55
Q

Solvent

A

substance that is doing the dissolving.

56
Q

Solution

A

substance that created as a mixture when the solute is dissolved by the solvent.

57
Q

Magnetic

A

the capability of being attracted by or acquiring the properties of a magnet.

58
Q

Flammability

A

the ease of which a combustible substance can be ignited that will result in a fire or even an explosion.

59
Q

Flashpoint

A

the lowest liquid temperature at which, under certain standardized conditions, a liquid gives off vapors in a quantity such as to be capable of forming an ignitable vapor/air mixture.
Lower F.P. = More Flammable.

60
Q

Toxicity

A

a measurement of the dosage needed of a substance to damage a particular organism.
Lower LD50 = more lethal.
ex. the LD50 for Cyanide is 4mg/kg. If the mass of a human adult is appx. 75kg, then 300mg of Cyanide is considered a lethal dose.

61
Q

Radioactivity

A

the instability and breakdown of the nucleus for an element’s atom.

62
Q

Electromagnetic Spectrum

A

a range of electromagnetic radiation that is organized based on frequency and wavelength.

63
Q

Color

A

the aspect of any object that may be described in terms of hue, lightness, and saturation.

64
Q

Wavelength

A

the distance between the crest (or trough) of two successive waves.

65
Q

Frequency

A

the amount of waves for a particular measurement of time.

66
Q

Achromatic

A

refracted light without the dispersion into its constituent colors. When all colors are both absorbed and reflected, the achromatic color is white. When all colors are absorbed but not reflected, the achromatic color is black.

67
Q

Albedo Effect

A

the ability for a surface to reflect sunlight; a form of radiation. White has high albedo whereas black has low albedo. This is why if you want to stay cool on a hot summer, it makes sense to wear white. All wavelengths of energy are absorbed and immediately being reflected.

68
Q

Emission

A

The range of wavelengths that are emitted by an atom or compound stimulated by either heat or light.

69
Q

Absorption

A

The range of wavelengths that are absorbed by an atom or compound stimulated by either heat or light.

70
Q

Quantum of energy

A

is the minimum amount of energy that can be lost or gained by an atom.

71
Q

Photon

A

a particle of light defined as a quantum of electromagnetic energy.

72
Q
A

Honors Chemistry (6 decks)

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