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Physical Science Benchmark 2 > Benchmark 4 Study Guide > Flashcards

Benchmark 4 Study Guide Flashcards

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0
Q

The most penetrating type of radiation.

A

Gamma

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1
Q

Negatively charged particles emitted from a nucleus at high speed.

A

Beta

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2
Q

The amount of time it take for half of a radioactive isotope to break apart.

A

Half-Life

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3
Q

The process by which nuclei having low masses are united to form nuclei with larger masses.

A

Fusion

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4
Q

Atoms of the same element with a different number of neutrons.

A

Isotope

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5
Q

Stopped by a piece of paper, a helium nucleus that is the weakest form of radiation.

A

Alpha

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6
Q

The splitting apart of a nucleus of a large atom into two smaller atoms.

A

Fission

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7
Q

Group18, inert, do not rom compounds

A

Noble Gases

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8
Q

The most reactive group of metals.

A

Alkali Metals

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9
Q

Elements that form salts by combining with metals.

A

Halogens

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10
Q

Includes oxygen and sulfur

A

Chalcogens

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11
Q

React to form bases, found in minerals

A

Alkaline Earth Metals

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12
Q

Form multiple charges, used to make pigments

A

Transition Metals

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13
Q

Found on the stair step line; part metal part nonmetal

A

Noble Gases

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14
Q

What does the chemical symbol represent for an element?

A

Name

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15
Q

This shows the number of elements in a compound and how they are bonded together.

A

Chemical Formula

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16
Q

What do dot diagrams represent?

A

Valence Electrons

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17
Q

What kind of chemical bond is formed when an equal exchange or transfer of electrons occurs.

A

Ionic

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18
Q

Hold atoms together in a compound

A

Chemical Bond

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19
Q

A group of covalently bonded atoms that acts together as one charged atom.

A

Polyatomic Ion

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20
Q

This is an abbreviation used for elements in chemistry.

A

Chemical Symbol

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21
Q

A chemical bond that occurs when atoms share electrons.

A

Covalent

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22
Q

What is an insoluble compound that forms during a chemical reaction?

A

Precipitate

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23
Q

Numbers that precede chemical formulas, used to balance equations.

A

Coefficients

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24
Q

H2O (l)

A

Liquid

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25
Q

Represent oxidation numbers or charges of ions

A

Superscripts

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26
Q

Dissolved in water (aq)

A

Aqueous

27
Q

O2(g)

A

Gas

28
Q

The number of each type of atom in the compound is shown by these numbers.

A

Subscripts

29
Q

Na (s)

A

Solid

30
Q

When two elements or compounds combine to make one large compound.

A

Synthesis

31
Q

When one element replaces another element in a compound.

A

Single Displacement

32
Q

When a compound splits apart into smaller compounds or elements.

A

Decomposition

33
Q

When a carbon compound reacts with oxygen to form heat, carbon dioxide, and water.

A

Combustion

34
Q

When an element gains electrons.

A

Reduction

35
Q

When an element loses electrons.

A

Oxidation

36
Q

When two salts react, break apart, and recombine to make two new compounds.

A

Double Displacement

37
Q

When a strong acid reacts with a strong base to produce water and salt.

A

Acid Base Neutralization

38
Q

Sodium Chloride

A

NaCl

39
Q

Mg(NO3)2

A

Magnesium Nitrate

40
Q

The sum of the oxidation numbers in a neutral compound.

A

Zero

41
Q

The mass of products must equal the mass of reactants.

A

Loa of Conservation of Mass

42
Q

The particles of matter that make up protons and neutrons.

A

Quarks

43
Q

Copper(ll) Sulfate

A

CuSO4

44
Q

Br2, I2, N2, Cl2, H2, O2, F2

A

Diatomic Molecules

45
Q

The only metal that is a liquid at room temperature.

A

Mercury

46
Q

A(n)____ chemical equation has the same number of atoms of each element on each side of the equation.

A

Balanced

47
Q

Each substance on the left of the arrow in a chemical equation is a __

A

Reactant

48
Q

Which of the following is a balanced chemical equation?

A

AnNO3 + NaCl>AgCl + NaNO3

49
Q

The energy required to break the original bonds is less than the energy release when new bonds form a(n) ___ reaction.

A

Exergonic

50
Q

If heat must be added to a chemical reaction for the reaction to take place, the reaction is _____.

A

Endothermic

51
Q

What type of reaction is shown in the following chemical equation: NH3 + HCL > NH4Cl?

A

Synthesis

52
Q

Which of the following could represent a decomposition reaction?

A

Compound = element + element

53
Q

In a chemical equation, the symbol that means dissolved in water is __.

A

(aq)

54
Q

When one element replaces another element in a compound, the reaction is a ___ reaction.

A

Single-displacement

55
Q

A substance that speeds up a

Chemical reaction without being permanently changed itself is a(n) ___.

A

Catalyst

56
Q

The breaking down of a substance into two or more simpler substances is ____.

A

Decomposition

57
Q

Each substance to the right of the arrow in a chemical equation is a(n) ___.

A

Product

58
Q

Substances that prevent, or slow down, chemical reactions are called ___.

A

Inhibitors

59
Q

A chemical reaction in which heat energy is released is ___.

A

Exothermic

60
Q

Numbers that precede symbols and formulas in a chemical equation are ___.

A

Coefficients

61
Q

According to the law of conservation of mass, how does the mass of the products in a chemical reaction compare to the mass of the reactants.

A

The masses are equal.

62
Q

What is an insoluble compound that forms during a chemical reaction?

A

Precipitate

63
Q

A chemical reaction in which two or more substances combine to form another substance is called a ____.

A

Synthesis reaction

64
Q

The burning of wood in a campfire that produces heat and light would be both an ____ and an ____ reactions.

A

Exergonic, exothermic

65
Q

When most chemical reactions take place, some ___ in the reactants must be broken, a process that requires energy.

A

Chemical bonds

66
Q

Copper (ll) plus sodium iodide yields Copper (ll) iodide plus sodium sulfate is represented by which balanced equation?

A

CuSO4 + 2 NaI > Na2SO4 + CuI2

Physical Science Benchmark 2 (4 decks)

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