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Chemistry 115 > Exam #1 > Flashcards

Exam #1 Flashcards

Study terms for the first exam (77 cards)

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1
Q

C_10_H_22_

A

Decane

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2
Q

How to write ionic compound formulas

A

1) Determine what the cation is and its charge 2) Determine what the anion is and its charge 3) Find the smallest number of cations and anions necessary to give you a neutral compound 4) Use those numbers as subscripts

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3
Q

A substance that does not conduct electricity when dissolved in water; most molecular compounds are this

A

Non-electrolyte

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4
Q

Sum of the atomic weights of all the atoms in a molecular compound

A

Molecular weight

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5
Q

Constitutional isomers of straight-chain alkanes in which at least one carbon atom is bound to 3 or 4 other carbons

A

Branched alkanes

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6
Q

Form stable ions that have different charges

A

Transition metals

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7
Q

Ions with two or more atoms

A

Polyatomic ions

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8
Q

The mass of a substance in one mole of a compound; 1) Find the mass of the substance in one mole of the compound 2) Divide the mass by the mass of one mole of the compound and multiply by 100

A

Percent composition

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9
Q

The number of protons in an atom’s nucleus; located above the symbol, it defines the elements

A

Atomic number

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10
Q

C_7_H_16_

A

Heptane

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11
Q

Lustrous and brittle; semiconductors; reactivity is similar to nonmetals but not as strong

A

Metalloids

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12
Q

Most reactive metals (violently with water); always found in ionic compounds

A

Alkali metals

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13
Q

The sum of products of the fractional abundances and their isotopic masses

A

Atomic weight

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14
Q

Atoms with the same atomic number but different mass numbers

A

Isotopes

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15
Q

The elements that are the building blocks of the body (all others are dietary minerals)

A

H, O, C, and N

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16
Q

The total number of protons and neutrons in an atom; located below the symbol, it approximates the mass of the atom

A

Mass number

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17
Q

A _____ ion is formed when an atom either gains or loses electrons

A

Monatomic ion

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18
Q

Group 18; Noted for their lack of reactivity; all exist as gases

A

Nobel (inert) gases

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19
Q

A molecular formula written in a way that shows how the atoms are grouped together in a molecule; CH_3_CH_2_CH_2_CH_3_

A

Condensed formula

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20
Q

The simplest (smallest) ratio of atoms in a molecule

A

Empirical formula

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21
Q

An atom or group of atoms that give particular properties and distinguishes different classes of organic compounds

A

Functional groups

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22
Q

Lower melting points than transition metals; softer than other metals; more cunductive than metalloids; higher boiling points than metalloids

A

Poor metals

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23
Q

Alkanes that form a ring

A

Cyclic alkanes

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24
Q

Compounds with the same molecular formula that differ in the order in which their atoms are bonded

A

Constitutional isomers

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25
Ionic compounds that have water molecules trapped within their crystal lattices
Ionic hydrates
26
Specifies the number of atoms of each element in a molecule: C\_6\_H\_12\_0\_6\_
Molecular formula
27
Organic compound that contains only carbon and hydrogen
Hydrocarbon
28
C\_3\_H\_8\_
Propane
29
Avogadro's Number
6.022 x 10(^23) per mole
30
Compounds with the same molecular formula but different atomic arrangements
Isomers
31
True or false: Metals usually form ionic compounds with non-metals
True
32
The molecular formula for straight-chain and branched alkanes
C\_n\_H\_2n+2\_
33
How to name a cyclic alkane
Add the prefix "cyclo-" to the ring(s), and name according to the rules for branched and straight-chain alkanes
34
Group 6A (16); ion charge of -2 (For O, S, Se, Te)
"Chalcogens"
35
How to name a branched alkane
1) Find the longest chain and name it according to the rules for straight-chain alkanes 2) Name each side chain by changing the suffix from "-ane" to "-yl" 3) Number the carbons of the longest chain beginning with the end that is closest to a side chain 4) Write the name of the alkane by arranging the names of the alkyl groups in alphabetical order (each preceded by the carbon number to which it is attached) and then name the stem 5) If there are multiple side chains of the same type, use the prefixes "di-", "tri-", "tetra-", "penta" and so forth to indicate this
36
Formed by the electrostatic (or Coulombic) attraction between cations and anions; solid form is crystal lattice
Ionic compounds
37
The mass of a particular isotope of an element (in atomic mass units)
Isotopic mass
38
Good conductors; malleable (can be rolled into sheets); ductile (can be drawn into wires); lustrous (shiny); Ten to be solids (-mercury)
Metals
39
Group 5A (15); Ion charge of -3 (for N, P, As, and Sb)
"pnictogens"
40
A compound that contains carbon
Organic compound
41
C\_9\_H\_20\_
Nonane
42
The molecular formula for cyclic alkanes
C\_n\_H\_2n\_
43
C\_4\_H\_10\_
Butane
44
The joining, separating, or rearranging of atoms
Chemical reaction
45
Ion charge of +3 (For B, Al, Ga, Ln; Ion charge of +1 (for Tl)
Group 3A (13)
46
How to name binary inorganic molecular compounds
1) Hydrogen always precedes the other element 2) The element listed furthest to the right on the periodic table is listed second and the suffix "-ide" is added to its root name 3) Indicate the number of atoms per element with Greek prefixes (mono-, di-, tri-, tetra-, penta-, hexa)
47
The decimal form of the percent abundance
Fractional abundance
48
Exactly the number of (^12)C atoms in 12 g of (^12)C
Mole
49
Have no net charge
Atoms
50
C\_6\_H\_14\_
Hexane
51
Hydrocarbons that only have single bonds between carbon atoms
Alkanes
52
Shows how different atoms are bound to each other
Structural formula
53
The percentage of an element that comes from a particular isotope
Percentage abundance
54
How to find the molecular formula
1) Find the molar mass of the fragment from the empirical formula 2) Divide the molar mass of the total compound by the molar mass of the fragment 3) Multiply all the subscripts in the empirical formula by the integer you get
55
Group 8A (17); Ion charge of -1 (for all halogens)
"Halogens"
56
Number of protons - number of electrons
Net charge
57
A substance that conducts electricity when dissolved in water (if it can dissolve in water, it is this)
Electrolyte
58
The total number of protons and neutrons; accounts for most of the atom's mass
Nucleus
59
The unit of molar mass
g/mol
60
How to write the names of ionic compounds
1) Write the cation name first 2) If the cation is a transition metal, write the charge in Roman numerals in parentheses immediately after the ion name 3) With monatomic anions, the anion name is the stem of the element name and the suffix "-ide"
61
A unit of matter in which two or more elements are chemically (covalently) bound
Molecular compound
62
Sum of the atomic weights of all the atoms in an ionic compound
Formula weight
63
CH\_4\_
Methane
64
C\_5\_H\_12\_
Pentane
65
How to calculate empirical formulas (Using percent compositions to calculate empirical formulas)
1) Assume that you have a 100 g sample 2) Determine the number of moles of each element in the sample 3) Divide all the number of moles of each element by the smallest value 4) Either multiply by a factor or round numbers to get whole numbers
66
Molecular compounds that do not contain carbon
Inorganic molecular compounds
67
Ions formed when one atom gains or loses electrons
Monatomic ions
68
Alkanes that exist as "linear" chains
Straight-chain alkane
69
The mass in grams of one mole of a substance
Molar mass
70
Protons and neutrons are nearly ______ more massive than electrons
2000 times
71
C\_8\_H\_18\_
Octane
72
Poor conductors; tend to be gases or liquids; Brittle (when solid); Can form molecules in covalent bonds or ionic compounds with metals
Non-metals
73
2nd most reactive metals (strongly with water); found in ionic compounds
Alkaline earth metals
74
The mass (in grams) of one mole of a compound; same as the molecular/formula weight; units are g/mol
Molar mass
75
C\_2\_H\_6\_
Ethane
76
Have either a positive or negative net charge
Ions
77
The most common elements in the body
H, O, C, N, Ca, P, S, Na, K, Cl, and Mg

Chemistry 115 (4 decks)

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