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Chem Vocab > Chem: Sec 1-2 (Essential Ideas, Atoms, Molecules, & Ions) > Flashcards

Chem: Sec 1-2 (Essential Ideas, Atoms, Molecules, & Ions) Flashcards

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1
Q

Chemistry is considered what type of Science?

A

Central Science: due to its link with biology, nuclear science, physics, material science, agriculture, medicine, geology, and host of other branches of science.

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2
Q

Chemistry is the study of?

A

Composition, properties, and interactions of matter.

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3
Q

Chemistry is mainly based on?

A

Observation and experimentation, in order to try and explain the behavior of chemical substances.

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4
Q

The experimentation in Chemistry is done in a systematic way, known as?

A

The Scientific Method: an approach to knowledge that begin and ends with observation.

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5
Q

Hypothesis is?

A

A tentative interpretation or unsure explanation of observation.

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6
Q

Experimentation is?

A

highly controlled procedures designed to generate scientific observations.

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7
Q

Scientific Law is?

A

A brief statement that summarizes past observations and predicts future ones.
(A consistently ‘proven’ fact that is withheld through the Science community.)

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8
Q

A Theory is?

A

A model for the way nature is, which tries to explain not only WHAT nature does, but WHY it does it.

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9
Q

Macroscopic domain considers?

A

Everyday things that we can see and touch.

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10
Q

Microscopic domain consists of?

A

Particles so small that they cannot be seen through a light microscope, but can be VISUALIZED using instruments such as tunneling electron microscopes.

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11
Q

What is Matter?

A

Anything that has mass and occupies space. Other acceptable answers : (Nothing, whats matter with you?)

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12
Q

Solids are defined as?

A

A form of matter in which the atoms or molecules are packed closely together in FIXED locations.

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13
Q

Liquids are defined as?

A

A form of matter in which atoms or molecules are packed almost as closely as in solids, but the particles are FREE TO MOVE relative to one another.

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14
Q

Gases are defined as?

A

A form of matter in which there is a lot of space between the atoms or molecules, and FREEDOM of movement.

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15
Q

Plasma is defined as?

A

A fourth state of matter which is similar to gases, but has large number of electrically charged particles.

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16
Q

What is Mass?

A

The quantity of matter within an object. (Distinct from weight, not the gravitational pull on the object.)

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17
Q

Pure Substances are?

A

A sample with a CONSTANT composition throughout and the same make-up and properties as other samples of the same substance, regardless of its source. (Only has one type atom or molecules.)

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18
Q

Elements are?

A

The simplest building block of matter. They cannot be chemically broken down into smaller substances.

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19
Q

Mixtures are?

A

Made up of TWO or MORE substances mixed together.

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20
Q

Heterogeneous Mixtures are?

A

Composition which is DIFFERENT from place to place in the sample.

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21
Q

Homogeneous Mixtures (Solutions) are?

A

Composition that is the SAME throughout the sample. (Different from pure substance, since mixture can have a VARIABLE composition.)

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22
Q

What is an Atom?

A

The smallest particle of an element that can enter into a chemical combination.

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23
Q

What are Molecules?

A

Two or MORE atoms held together by chemical bonds.

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24
Q

Compounds are?

A

Chemical combinations of two or more elements.

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25
Q

Physical properties are?

A

Properties of a substance observed without the substance undergoing a change in composition. Ex. (Color, odor, boiling point, density.)

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26
Q

Physical Change is?

A

The Process in which matter changes its appearance, but NOT composition. Ex. (Crushing, and Phase Change.)

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27
Q

Chemical Properties are?

A

Observed when a substance undergoes a change in composition (formula.) Ex. (Chemical reaction resulting in new bonds/formula.)

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28
Q

Chemical Change is?

A

A process in which matter DOES change its composition. Ex. (Burning, rusting, since a new compound or compounds are formed during the process.)

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29
Q

Extensive Properties depend on?

A

The AMOUNT of substance in a sample. Ex. (Volume, mass, heat.)

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30
Q

Intensive Properties are?

A

Independent of the amount of substance in a sample. Ex. (Density, temperature, color.)

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31
Q

Kilo- (k) is?

A

10^3 = 1000 (one-thousand).
Ex. (1 km = 1000 m)

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32
Q

Mega- (M) is?

A

10^6 = 1,000,000 (one million.)
Ex. ( 1 Mb = 1,000,000 bytes)

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33
Q

Giga- (G) is?

A

10^9 = 1,000,000,000 (one billion)
Ex. ( 1 Gb = 1,000,000,000 bytes)

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34
Q

Tera- (T) is?

A

10^12 = 1,000,000,000,000 (one trillion)
Ex. (1 Tb = 1,000,000,000,000 bytes)

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35
Q

Deci- (d) is?

A

10^-1 = 0.1 = 1/10 (one tenth)
Ex. ( 1 dm = 0.1 meters)

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36
Q

Centi- (c)

A

10^-2 = .01 = 1/100 (one hundredth)
Ex. ( 1cm = .01 m)

37
Q

Mili- (m) is?

A

10^-3 = .001 = 1/1000 (one thousandth)
Ex. ( 1 mm = .001 m)

38
Q

Micro- (µ) is?

A

10^-6 = .0000001 = 1/1000000 (one millionth)
Ex. ( 1 ms = .0000001 s)

39
Q

Nano- (n) is?

A

10^-9 = .0000000001 = 1/1000000000 (one billionth)
Ex. ( 1 ns = .0000000001 s)

40
Q

1 mL = 1 cm^3

A

This refers to the conversion factor of volume from mL to cm. A base 1.

41
Q

Temperature conversion from C -> F?

A

(C • 1.8) + 32 = F.

42
Q

Temperature conversion from F -> C

A

(F - 32)/ 1.8 = C.

43
Q

Temperature conversion to Kelvin?

A

C+ 273.15 = K.
or
K - 273.15 = C.

44
Q

Density Form.?

A

D= m/v

45
Q

Sig. Fig says: When adding and subtracting, the result carries same number of what?

A

Same number of DECIMALS PLACES as the quantity carrying the FEWEST decimal places.

46
Q

Sig. Fig says: When multiplying and dividing, the result carries same number of what?

A

Same number of sig. figs. as the factor with the FEWEST sig. figs.

47
Q

Accuracy in Chemistry refers to?

A

The closeness of the measured value to the actual value.

48
Q

Precision in Chemistry refers to?

A

The closeness of a series of measured values to one another.

49
Q

Dimensional Analysis/ Factor- Label Method is?

A

The use of units as a guide to solving problems.

50
Q

Unit conversion factors are?

A

Factors formed from a relationship, such as 1 in. = 2.54 cm can be written as 1 in./ 2.54 cm. or 2.54 cm./ 1 in.

51
Q

The Law of definite Proportion (matter is neither created nor destroyed during reaction) was discovered by who in 1797?

A

Joseph Proust

52
Q

The Law of Multiple Proportion states?

A

When two elements form two different compounds, the masses of Element B that combine with one gram of Element A can be expressed as a ratio of small whole numbers.

53
Q

What are Electrons?

A

Negatively charged particles found outside the nucleus. (Protons and electrons are usually balanced, so the atom is electrically neutral.)

54
Q

What is Radioactivity?

A

The emission of small energetic particles from the core of unstable atoms. (its discovery allowed the structure of the atom to be probed using alpha particles).

55
Q

Atomic Theory: the model of the atom was proposed by who?

A

Ernest Rutherford in 1909.

56
Q

The Nucleus is?

A

The small core of the atom which contains most of its mass and all of its positive charge.

57
Q

The Proton is?

A

A positively charged particle found in the nucleus of the atom. (Protons and electrons are always balanced, so the atom is electrically neutral.)

58
Q

What are Isotopes?
(Not the Baseball team.)

A

Different versions of the same element having different masses, but chemically indistinguishable.
Ex. ^12C, ^13C, ^14C (same atomic numbers different mass number)

59
Q

What are Neutrons?

A

A neutral particle found in the nucleus of an atom.

60
Q

Atomic Mass Unit (amu) =

A

Approximately 1.67 x 10^-24 g.

61
Q

Fundamental Unit of Charge (C) =

A

1.602 x 10^-19 C.

62
Q

Atomic number (z) refers to?

A

The number of PROTONS in the nucleus. Determines the identity of the atom. It is the integer found at the top of each “box” in the periodic table.

63
Q

Mass number (A) refers to?

A

The total number of PROTONS and NEUTRONS in an atom.

64
Q

What are Ions?

A

A charged particle formed when an atom LOSES or GAINS one or more electrons.

65
Q

What is an Anion?

A

An ion formed when an atom GAINS one or more electrons. Anions are negatively charged.
Ex. F- ,O2- ,S2-, Cl-.

66
Q

What is a Cation?

A

An ion formed when an atom LOSES one or more electrons. Cations are positively charged.
Ex. Li+, Ca2+, Na+, Al3+.

67
Q

What is Atomic Mass?

A

The average mass of an element.
Ex. Atomic mass = (Amu isotope 1 x natural abundance(1)) + (Amu isotope 2 x natural abundance(2)) + etc.

68
Q

What is Molecular Form.?

A

A representation of a molecule using chemical symbols to represent the type of atoms in the compound, and subscripts to indicate the number of atoms of each type in the compound.

69
Q

What is Structural Form.?

A

Similar to molecular form., but shows how the atoms are connected to one another.

70
Q

What is Empirical Form.?

A

The SIMPLEST whole- number ratio of atoms to each other in a compound.
Ex. C6H12O6 -> CH2O

71
Q

What are Structural Isomers?

A

Compounds with the same formula, but in which the atoms are connected to each other in different ways.

72
Q

What are Special Isomers?

A

Compounds in which the atoms are oriented differently in 3 dimension.

73
Q

The horizontal rows on the Periodic Table are called?

A

Periods or Series.

74
Q

The vertical columns on the Periodic Table are called?

A

Groups.

75
Q

Where are Metals found?
How are they identified?

A

Elements found in the middle and lower left side of the periodic table. They are good conductors, shiny, ductile (stretchable), malleable (bendable), and tend to LOSE electrons in chemical reactions.

76
Q

Where are Nonmetals found?
How are they identified?

A

Elements found in the upper right of the periodic table. They have varying properties, but are poor conductors of heat and electricity, and they tend to GAIN electrons in chemical reactions.

77
Q

Where are Metalloids found?
How are they identified?

A

Elements found in the zigzag diagonal line that divides metal from nonmetals. Their properties are between those of metals and nonmetals, and some of them are semi- conductors, due to their intermediate electrical conductivity.

78
Q

What groups are the Representative Elements found in?

A

Groups “A” (1-2 & 13-18)
(IA, IIA, IIIA, IVA, VA, VIA, VIIA, VIIIA)

79
Q

Where are Transition Metals found?
How are they identified?

A

Elements in the “B” (3-12) groups, whose properties are less predictable based on their position in the periodic table.
“Elements behaving badly.”

80
Q

Where are Noble Gases found?
How are they identified?

A

Elements in Group 18, 8A, (VIIIA) which are largely unreactive.

81
Q

Where are Alkali Metals found?
How are they identified?

A

Elements in Group 1, 1A, IA, which are very reactive. (Does not include H.)

82
Q

Where are Alkaline Earth Metals found?
How are they identified?

A

Elements in Group 2, 2A, IIA, which are fairly reactive.

83
Q

Where are Halogens found?
How are they identified?

A

Elements in Group 17, 7A, VIIA, which are very reactive nonmetals.

84
Q

What are Monoatomic Ions?

A

Ions formed from only one atom.

85
Q

What are Polyatomic Ions?

A

Ions form from several atoms- essentially a charged molecule.

86
Q

What are Oxyanions Polyatomic Ions?

A

Polyatomic Ions that have one or more oxygen atoms.

87
Q

What makes an Ionic Bond?

A

Electrostatic force of attraction that holds cations and anions together. (Typically between metals and nonmetals bonds.)

88
Q

What makes a Covalent Bond?

A

The attractive force between two atoms that share on or more electron pairs. (Typically found when two nonmetals bond.)

Chem Vocab (7 decks)

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