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PFigs Benchmark > Second semester > Flashcards

Second semester Flashcards

0
Q

Most penetrating type of radiation

A

Gamma

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1
Q

Negatively charged particles emitted firm a nucleus at high speed

A

Beta

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2
Q

Amount of time it takes 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 if a nucleus of a large atom into two smaller atoms

A

Fission

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7
Q

Group 18 inert do not form 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 for 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 in the stair step line part metal part nonmetal

A

Metalloids

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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 now 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 if chemical bond is formed when an equal exchange or transfer of electrons occur

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

Coefficient

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24
Q

H2O (l)

A

Liquid

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25
Q

Represent oxidation numbers or charges of ions

A

Subscripts

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26
Q

Dissolved in water

A

Aqueous

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27
Q

O2

A

Gas

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28
Q

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

A

Superscripts

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 and element gains and electron

A

Oxidation

35
Q

When an element loses an electron

A

Reduction

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 dune if the oxidation numbers in a neutral compound

A

Zero

41
Q

The mass of the product must equal the mad if the reactants

A

Law of conservation of mass

42
Q

Copper (II) sulfate

A

CuSO4

43
Q

Br2 i2 N2 Cl2 H2 O2 F2

A

Diatomic molecules

44
Q

The only metal that is a liquid at room temperature

A

Mercury

45
Q

⚪️+⚫️>⚪️⚫️

A

Synthesis

46
Q
A

Single decomposition

47
Q

⚫️

A

Decomposition

48
Q

⚪️⚫️+

A

Double displacement

49
Q

A_____ chemical equation has the same number if atoms of each element on each side of the equation

A

Balanced

50
Q

Each substance on the left side of the arrow in a chemical equation___.

A

Reactant

51
Q

Which of the following is a balanced chemical equation

A

AgNO3+2NaCl>AgCl+NaNO3

52
Q

The energy required to break the original bonds is less than the energy release when new bonds form in an____reaction

A

Endergonic

53
Q

If heat must be added to a chemical reaction for the reaction to take place the reaction is___

A

Endothermic

54
Q

What type if reaction is shown in the following chemical equation NH3+HCl>NH4Cl

A

Synthesis

55
Q

Which of the following could represent a decomposition reaction?

A

Compound=element+element

56
Q

In a chemical equation the symbol that means dissolved in water is___

A

(aq)

57
Q

When one element replaces another element in a compound the reaction is a ____reaction

A

Single displacement

58
Q

A substance that speeds up a reaction without being permanently changed itself is a___

A

Catalyst

59
Q

Each substance to the right of the arrow in a chemical equation is a__

A

Product

60
Q

The breaking down if a substance into two or more simpler substances is___

A

Decomposition

61
Q

Substances that prevent or slow down chemical reactions are called

A

Inhibitors

62
Q

A chemical reaction in which hear energy is released___

A

Exothermic

63
Q

Numbers that precede symbols and formulas in a chemical equation are___

A

Coefficient

64
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

65
Q

What is an insoluble compound that forms during a chemical reaction

A

Precipitate

66
Q

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

A

Synthesis reaction

67
Q

The burning of wood in a campfire that produces heat and light would be both an___and ____reaction

A

Exergonic and endothermic

68
Q

When most chemical reaction take place some____in the reactants must be broken a process that requires energy

A

Compounds

69
Q

Copper(II) sulfate plus sodium iodide yields copper (II) iodide plus sodium sulfate is represented by whose balanced equation

A

CuSO4+2NaI>NaSO4+CuI2

PFigs Benchmark (1 decks)

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