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Honors Chemistry > Semester 1 Terminology > Flashcards

Semester 1 Terminology Flashcards

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1
Q

Chemistry

A

The science that deals with the composition and properties of substances

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2
Q

Quantity

A

A property that can be measured and described by a number and unit.

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3
Q

SI System

A

The Standard International system for measurements, assures that scientists are using the same units when describing a quantity.

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4
Q

Scientific Notation

A

Expressing numbers by powers of ten

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5
Q

Significant Figures

A

The number of digits displayed for a calculated number, based on the number of digits used in the original information that is given or measured.

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6
Q

Assumption

A

A conclusion that may or may not be correct, usually a combination of personal belief and partial bits of evidence.

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7
Q

Atom

A

The smallest unit of matter

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8
Q

Element

A

A single type of atom, of which there are over 100 different types, based on the number of protons in the nucleus.

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9
Q

Compound

A

Chemically joined combinations of two or more atoms.

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10
Q

Pure Substance

A

Composed of the same substance throughout, even on the submicroscopic scale. Includes elements and chemically joined combinations of elements, compounds.

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11
Q

Mixture

A

Physically composed of many different substances; may appear to be a pure substance if mixed evenly, homogenous, or may be unevenly mixed, heterogeneous.

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12
Q

Law of definite composition of compounds.

A

Compounds are pure substances, that are made up of a definite ratio, or definite composition, of chemically joined elements.

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13
Q

Law of Multiple Proportions

A

The same elements that make one compound, can be joined together to make another completely different compound.

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14
Q

Molecular Compounds

A

Function as independent particles; a compound where the ration of elements states how many of each element are actually in each independent molecule.

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15
Q

Ionic Compounds

A

Function as a crystal lattice of particles; a compound where the ratio of elements states only the lowest common ratio, or the smallest crystal lattice of articles possible.

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16
Q

Formula Unit

A

Smallest unit of an ionic compound’s network or crystal lattice.

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17
Q

Ion

A

An element or compound with a charge. Due to loss or gain of electrons.

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18
Q

Cation

A

Positive (+) ion due to loss of electrons

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19
Q

Anion

A

Negative (-) ion due to gain of e

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20
Q

Polyatomic Ions

A

Ions composed of many elements; a combination of elements with a charge.

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21
Q

Alloy

A

A mixture of two or more metals.

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22
Q

Chemical Reaction

A

When pure substances chemically combine or break apart to form new pure substances.

23
Q

Energy

A

The ability to do work or give off heat.

24
Q

Law of Conservation of Mass

A

In a closed or isolated system, matter cannot be created or destroyed. It can change forms but is conserved.

25
Q

Kinetic Energy

A

Movement, or work, related energy

26
Q

Potential Energy

A

Stored Energy

27
Q

Law of Conservation of Energy

A

Energy can neither be created nor destroyed - only converted from one form of energy to another.

28
Q

System

A

The set of substances and energy that is being studied

29
Q

Surroundings

A

What is in contact with the system.

30
Q

Exothermic

A

Heat leaves the system

31
Q

Endothermic

A

heat enters the system

32
Q

Combustion

A

An exothermic reaction in which a substance combines with oxygen to form products in which all elements are combined with oxygen. (Usually contains Carbon and Hydrogen and produce CO2 and H2O)

33
Q

Composition and Decomposition

A

Reactions that are putting together or taking apart a substance.

34
Q

Single Replacement Reactions

A

A metal replaces a metal or hydrogen in a compound, or a nonmetal replaces a nonmetal in a compound, based on their activity levels.

35
Q

Double Replacement Reactions

A

involves the switching of cations and anions for two aqueous compounds.
AB + CD -> AD +CB

36
Q

Ionic Equation

A

a chemical equation where soluble compounds are shown as ions

37
Q

Net ionic Equation

A

Ions that appear on both sides of the ionic equation are not shown

38
Q

Avogadro’s Number

A

6.022 × 10²³
The number of atoms in 12 grams of carbon 12

39
Q

Mole

A

Avogadro’s number, usually in reference to atoms, molecules or particles which can be converted from grams to moles based on their respective atomic mass.

40
Q

Atomic Mass

A

The weighted average mass of the isotopes of an element.

41
Q

Molar Mass

A

The mass in grams of one mole of a pure substance

42
Q

Percent

A

Parts Per hundred

43
Q

Percent Composition (Percent mass)

A

How much of each component is in a mixture or compound.

44
Q

Empirical Formula

A

It is the lowest ratio of elements in a compound found from the experimental data.

45
Q

Molecular Formula

A

The actual formula of a compound; may be the same or multiple of the Empirical.

46
Q

Molarity

A

Concentration expressed in moles per Liter.
Mol/L

47
Q

Stoichiometry

A

Derived from Greek - “to measure elements” Involves measuring or Calculating the amounts of elements or compounds involved in a chemical change.

48
Q

Limiting Reactant

A

The reactant that limits the amount of product that can be made.

49
Q

Excess reactant

A

The reactant that will still be left over when the limiting reactant is completely consumed.

50
Q

Theoretical Yield

A

Amount of product predicted based on balanced chemical equation.

51
Q

Actual Yield

A

The amount of product yielded in a reaction, according to real measurements.

52
Q

Percent Yield

A

The efficiency of a reaction described by the actual yield divided by the theoretical yield.

53
Q

STP

A

Standard temperature and pressure. Gases have approximately 22.4 L/mol at STP. Because the number of particles of a gas changes with both temperature and pressure a predetermined value for temperature and pressure is needed in order to make a useful conversion.

Honors Chemistry (1 decks)

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