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science flash cards 7th > quarter 1 > Flashcards

quarter 1 Flashcards

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1
Q

The temperature at which a liquid changes into a gas.

A

Boiling Point

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2
Q

The change from a gas to a solid. Requires removing energy so the particles slow down.

A

deposition

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3
Q

The particles are very far apart and they move freely and quickly. It has no definite shape or volume so it can take on both the shape and volume of its container.

A

Gas

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4
Q

The change from a gas to a liquid. Requires removing energy so the particles slow down.

A

Condensation

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5
Q

The change from a liquid to a solid. Requires removing energy so the particles slow down.

A

Freezing

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6
Q

The temperature at which a liquid changes into a solid.

A

Freezing Point

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7
Q

A graphical representation of how the state of matter changes in response to temperature change.

A

Heating Curve

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8
Q

The particles are close together and they vibrate, move, and slide past each other. It has a definite volume but no definite shape so it can take on only the shape of its container.

A

Liquid

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9
Q

The change from a solid to a liquid. Requires adding energy so the particles speed up.

A

Melting

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10
Q

The temperature at which a solid changes into a liquid.

A

Melting Point

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11
Q

A graphical representation that shows the temperature and pressure conditions in which a phase of matter will exist

A

Phase Diagram

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12
Q

Forms when a gas becomes hot enough for the energy to separate the particles in the atoms. Made up of free ions and negative electrons.

A

Plasma

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13
Q

The particles are tightly packed together and they vibrate in place. Has a definite shape and volume so it does not easily change shape or volume.

A

Solid

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14
Q

The change from a solid to a gas. Requires adding energy so the particles speed up.

A

Sublimation

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15
Q

The change from a liquid to a gas. Requires adding energy so the particles speed up.

A

Vaporization

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16
Q

Group 1: 1 valence electron. Extremely reactive

A

Alkali Metals

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17
Q

Group 2: 2 valence electrons. Very reactive (slightly less reactive than group 1).

A

Alkaline-Earth Metals

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18
Q

Basis for arranging elements on the modern Periodic Table. Tells the number of protons for each element.

A

Atomic Number

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19
Q

Size of an atom. Measured from the center of the nucleus to the outermost energy level.

A

Atomic Radius

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20
Q

an expression that shows the elements in a compound and the relative proportions of those elements

A

Chemical Formula

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21
Q

a one or two letter abbreviation to represents an element

A

Chemical Symbol

22
Q

A group of elements with similar chemical and physical properties.

A

Family

23
Q

Most reactive nonmetal.

A

Fluorine

24
Q

Most reactive metal.

A

Francium

25
Q

A vertical column in the periodic table. Indicates the number of valence electrons.

A

Group

26
Q

Group 17: 7 valence electrons. Extremely reactive.

A

Halogens

27
Q

Lower two rows of the periodic table. Lanthanides and actinides. Some are radioactive (unstable).

A

Inner Transition Metals

28
Q

Also known as semi-metals. Share properties of metals and nonmetals. Semiconductors.

A

Metalloids

29
Q

Located on the left side. Largest group of elements. Most are solid at room temperature, shiny, good conductors of electricity, malleable, and ductile.

A

Metals

30
Q

Group 18: 8 valence electrons (Helium has 2). Nonreactive.

A

Noble Gases

31
Q

Located on the right side. Second largest group of elements. Most are gases at room temperature, dull, poor conductors of electricity, not malleable, and not ductile.

A

Nonmetals

32
Q

A horizontal row in the periodic table. Indicates the number of energy levels.

A

Period

33
Q

Organization of all known elements by increasing atomic number and physical/chemical properties

A

Periodic Table

34
Q

Groups 3-12: 1-2 valence electrons. Slightly reactive (less than group 2).

A

Transition Metals

35
Q

Electrons in the outermost energy level of an atom. Determines the reactivity of an atom.

A

Valence Electrons

36
Q

A property of matter that describes a substance’s ability to participate in chemical reactions.
Corrosiveness

A

Chemical Property

37
Q

The ability of a substance to damage or destroy another substance it comes into contact with. (rusting, tarnishing, oxidation)

A

Corrosiveness

38
Q

The ability of a substance to damage or destroy another substance it comes into contact with. (rusting, tarnishing, oxidation)

A

Corrosiveness

39
Q

The amount of mass in a given volume (D = m/v)

A

Density

40
Q

The ability to be pulled into thin wires.

A

Ductility

41
Q

A measure of the tendency of an atom to attract electrons.

A

Electronegativity

42
Q

The ability of a substance to burn.

A

Flammability

43
Q

The ability of a substance to be hammered or rolled into sheets.

A

Malleability

44
Q

The tendency of atoms to prefer to have 8 valence electrons.

A

Octet rule

45
Q

A chemical change in which a substance combines with oxygen.

A

Oxidation

46
Q

A characteristic of a pure substance that can be observed or measured without changing the identity of the substance.

A

Physical property

47
Q

The property that describes how readily a substance combines chemically with other substances.

A

Reactivity

48
Q

The corrosion of Iron.

A

Rusting

49
Q

The ability to dissolve in another substance.

A

Solubility

50
Q

The corrosion of a metal.

A

Tarnishing

51
Q

The ability of an object to transfer heat.

A

Thermal conductivity

52
Q

A liquid’s resistance to flowing.

A

Viscosity

science flash cards 7th (4 decks)

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