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Chem 101 > Chapter 2 > Flashcards

Chapter 2 Flashcards

(63 cards)

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1
Q

Law of Definite Proportions

A

different samples of a given compound always contain the same elements in the same mass ratio

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2
Q

Law of Multiple Proportions

A

if two elements can combine to form more than one compound with each other, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers

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3
Q

Law of Conservation of Mass

A

matter can neither be created or destroyed

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4
Q

Atom

A

the basic unit of an element that can enter into chemical combination

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5
Q

Radiation

A

the emission and transmission of energy through space in the forms of waves

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6
Q

Cathode Ray Tube

A

used to investigate atomic structure

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7
Q

Coulomb

A
  • the derived S.I. unit of electric charge
  • 1 Coulomb=1 (Ampere)(second)
  • 1.76x10^8 Coulombs/gram
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8
Q

Charge of Electron

A

-1.6022x10^-19 Coulombs

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9
Q

Mass of Electron

A

9.10x10^-28 grams

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10
Q

Radioactivity

A

describes the spontaneous emission of particles and/or radiation

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11
Q

Alpha Rays

A

consist of positively charged particles called “alpha particles” that are deflected away from the positively charged plate in the Cathode Ray Tube

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12
Q

Beta Rays/Particles

A

are electrons, so they are deflected away from the negatively charged plate in the Cathode Ray Tube

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13
Q

Gamma Rays

A

high-energy, have no charge and are unaffected by external electric or magnetic fields

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14
Q

Rutherfords Experiment

A

plum pudding model –> nuclear model

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15
Q

Nucleus

A

an extremely dense central core within the atom

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16
Q

Protons

A

the positively charged particles in the nucleus

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17
Q

Mass of Proton

A

1.67262x10^-24 grams

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18
Q

Charge of Proton

A

1.6022x10^-19 Coulombs

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19
Q

Picometer (pm)

A

1 pm=1x10^-12 m

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20
Q

Angstrom

A

1 Angstrom=1x10^-10 m

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21
Q

Atomic Number

A

the number of protons in the nucleus of each atom of the element. Also indicates the number of electrons because atoms are neutral

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22
Q

Mass Number

A

the total number of neutrons and protons present in the nucleus of an atom of an element

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23
Q

Nucleons

A

a particle within the nucleus

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24
Q

Isotopes

A

atoms that have the same atomic number but different mass numbers

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25
Periods
the elements are arranged by atomic number (above the element symbol) in horizontal rows
26
Groups/Families
vertical columns. Elements in the same group tend to have similar physical and chemical properties
27
Metal
a good conductor of heat and electricity
28
Nonmetal
a poor conductor of heat and electricity
29
Metalloid
has properties that are intermediate between those of metals and nonmetals
30
Groups on the Periodic Table of Elements: what are their names?
1. Alkali metals=group 1A-Hydrogen 2. Alkaline Earth metals=group 2A 3. Chalcogens=group 6A 4. Halogens=Group 7A 5. Noble Gases=Group 8A 6. Transition metals/elements=Groups 1B and Groups 3B-8B
31
Atomic Mass
the mass of an atom in atomic mass units
32
One Atomic Mass Unit (amu)
a mass exactly equal to one-twelfth the mass of one carbon-12 atom
33
Atomic Weight
sometimes used to mean average atomic mass
34
Monatomic Gases
exist in the form of isolated atoms under ordinary conditions. Only 6 noble gases
35
Molecule
a combination of at least two atoms in a specific arrangement held together by electrostatic forces known as covalent chemical bonds
36
Diatomic Molecule
consists of two atoms
37
Homonuclear Diatomic Molecules
both atoms in each molecule are of the same element
38
Heteronuclear Diatomic Molecules
contains atoms of different elements
39
Polyatomic Molecules
molecules containing more than two atoms
40
Chemical Formula
denotes the composition of the substance
41
Molecular Formula
shows the exact number of atoms of each element in a molecule
42
Allotrope
one of two or more distinct forms of an element. e.g. two of the allotropic forms of the element carbon are diamonds and graphite, which have dramatically different properties
43
Structural Formula
shows not only the elemental composition, but also the general arrangement of atoms within the molecule
44
Binary Molecular Compounds
substances that consist of just two different elements
45
Acid
a substance that produces hydrogen ions when dissolved in water
46
Ionizable Hydrogen Atom
one that separates from the molecule upon dissolving and becomes a hydrogen ion
47
Inorganic Compounds
generally defined as compounds that do not contain carbon
48
Organic Compounds
contain carbon and hydrogen, sometimes in combination with other elements such as oxygen, nitrogen, sulfur, and the halogens
49
Hydrocarbons
organic compounds that contain only carbon and oxygen
50
Alkane
the simplest examples of hydrocarbons. The name of alkane depends on the number of carbon atoms in the molecule
51
Functional Group
a group of atoms that replaces one of the hydrogen atoms. Determines many of the chemical properties of a compound because it typically is where a chemical reaction occurs
52
Greek prefixes: what are they?
``` mono=1 di=2 tri=3 tetra=4 penta=5 hexa=6 hepta=7 octa=8 nona=9 deca=10 ```
53
Ionic Bonds
strong electrostatic forces that hold ions together, making ionic compounds
54
Atomic Ions
an ion that consists of just one atom with a positive or negative charge A.K.A. monatomic ion
55
Cation
an ion with a net positive charge. Caused by the loss of one or more electrons
56
Anion
an ion whose net charge is negative due to the increase in the number of electrons
57
Ionic Compound
consists of cations and anions
58
Polyatomic Ions
ions that consist of a combination of two or more atoms. Held together by covalent chemical bonds
59
Lattice
interspersed cations and anions. Not discrete molecular units
60
Oxoanions
polyatomic anions that contain one or more oxygen atoms and one atom of another element
61
Oxoacids
ionize to produce hydrogen ions and the corresponding oxoanions
62
Polyprotic
oxoacids that have more that on ionizable hydrogen atom
63
Hydrates
compounds that have a specific number of water molecules within their solid structure

Chem 101 (2 decks)

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