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GenChem_ARC Flashcards

1
Q

It is anything that has mass and volume. It can be described by using physical and chemical properties.

A

Matter

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2
Q

These are properties that can be observed or measured.

A

Physical Properties

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3
Q
  1. Color
  2. Temperature
  3. Flammability
  4. Density
  5. Mass
  6. Length
  7. Volume
  8. Conductivity
  9. Reactivity
  10. State
A

Physical Property (PP) ; Chemical Property (CP)
1. PP
2. PP
3. CP
4. PP
5. PP
6. PP
7. PP
8. PP
9. CP
10. PP

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4
Q

These are properties that determine whether or not a substance will react chemically.

A

Chemical Properties

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5
Q

It does not depend on the size or amount of the sample.

A

Intensive Property

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6
Q

Also known as Intrinsic Property

A

Intensive Property

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7
Q

It depends on the size or amount of the sample.

A

Extensive Property

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8
Q

Also known as Extrinsic Property.

A

Extensive Property

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9
Q

Intensive or Extensive: Density

A

Intensive

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10
Q

It is the simplest substances. Made up of one atom.

A

Element

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11
Q

Made up of more than one type of atom.

A

Compound

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12
Q

The composition is uniform.

A

Homogenous mixture

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13
Q

The composition is not uniform.

A

Heterogeneous mixture

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14
Q

Each element is composed of extremely small particles called atoms. All the atoms of a given element are identical, but they differ from those of any other element.

A

Billiard Ball Model (1803)

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15
Q

Billiard Ball Model (1803)

A

Dalton

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16
Q

The atom is made up of negative electrons that float in a sphere of positive charge like plums in a pudding.

A

Plum Pudding Model (1904)

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17
Q

He discovered electron (cathode ray experiment) in 1897 and isotopes in 1913.

A

J.J. Thomson

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18
Q

Discovered the nucleus of a gold atom with his “gold foil” experiment.

A

Ernest Rutherford

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19
Q

The atom is mostly empty space. There is a small, dense center with a positive charge. Electrons in fixed orbit.

A

Nuclear Model (1911)

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20
Q

Nucleus surrounded by orbiting electrons at different energy levels. Electrons have definite orbits.

A

Bohr’s Planetary Model (1913)

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21
Q

Positive charge (+), 1
atomic mass unit (amu); found in
the nucleus.

A

Proton

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22
Q

Neutral charge (0), 1
amu; found in the nucleus.

A

Neutron

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23
Q

Negative charge (-),
mass is VERY small.

A

Electron

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24
Q

Its number determines the identity of the element.

A

Proton

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25
Atomic Number
Number of protons in nucleus.
26
Mass Number (Atomic Mass)
Number of protons + neutrons.
27
Atoms of the same element with varying number of neutrons.
Isotopes
28
Carbon has three naturally occurring isotopes with ______ having the highest percent abundance.
C-12
29
He arranged the elements in groups of 3’s or triads also known as Law of Triad (1829).
Johann Wolfgang Dobereiner
30
Arranged the elements in groups of 8’s or Law of Octaves (1894).
John Newlands
31
Recognized the repeating pattern or the periodic behavior among elements. He studied the relationship of the atomic volume and the relative atomic mass of 28 elements.
Julius Lothar Meyer
32
He formulated the Periodic Law.
Dmitri Mendeleev
33
The seven horizontal rows in the periodic table are called
PERIODS
34
The vertical columns are called
GROUPS or FAMILIES
35
Each element in the group has a completely filled set of s and p orbitals. All are colorless and exhibit little or no reactivity. Also known as inert gases.
Noble Gases
36
rare-earth elements
Lanthaniods
37
heavy rare elements
Actinoids
38
The average distance between nucleus and the valence electron.
Atomic Size (Atomic Radius)
39
It is the ability of the atom to donate electrons.
Metallic Property
40
Tendency of an atom to react.
Reactivity
41
The amount of energy required to remove an electron from an atom or ion.
Ionization Energy
42
The change in energy when an electron is accepted by a gaseous atom to form an anion.
Electron Affinity
43
Defined as the relative ability of an atom of an element to attract or gain electrons.
Electronegativity
44
The orbitals of an atom must be filled up in increasing energy levels.
Aufbau Principle
45
No two electrons in an atom can have the same set of quantum numbers and an atomic orbital must contain a maximum of two electrons with opposite spins.
Pauli’s Exclusion Principle
46
The most stable arrangement of electrons in subshells is the one with more parallel spins.
Hund’s Rule of Multiplicity
47
The average distance of the electron from the nucleus in a particular orbital.
Principal Quantum Number
48
It tells the shape of the orbital.
Azimuthal / Angular Momentum Quantum Number
49
It describes the orientation of orbital.
Magnetic Quantum Number
50
It shows the spin of electrons.
Spin Quantum Number (𝒎𝒔)
51
The forces of attraction that hold together atoms or ions when they combine to form molecules or ion pairs in a given compound.
Chemical bonds
52
An ionic bond is formed by actual electron-transfer; metal to non-metal.
Ionic Bonding
53
It is formed by electron sharing; non-metal to non-metal.
Covalent Bonding
54
One in which two or more substances (either elements or compounds) react to form one compound. General Form: A + B  AB
Composition reaction
55
One in which one compound decomposes to form two or more new substances. General Form: AB  A + B
Decomposition reaction
56
One in which a metal replaces another metal ion from a solution or a non metal replaces a less active non metal in a compound. General Form: AX + B  BX + A AX + Y  AY + X
Single replacement reaction
57
One wherein two compounds react to form two new compounds. General Form: AX + BY  AY + BX
Double decomposition reaction
58
substance that is oxidized
Reducing agent
59
substance that is reduced
oxidizing agent
60
The ratio of the total mass of each element to the total mass of one mole of the compound (MM) multiplied by 100%.
Percent Composition
61
Gives the simplest ratio of the number of moles of atoms.
Empirical Formula
62
Gives the actual ratio of the number of moles of atoms in a mole of the compound.
Molecular Formula
63
Homogeneous mixture of 2 or more substances.
Solution
64
dissolvingmedium
Solvent
65
dissolve substance
Solute
66
ability of a solvent to dissolve a salt at a particular temperature.
Solubility
67
solvent can still dissolve the solute.
Unsaturated Solution
68
if a solvent can’t no longer dissolve a given solute at a given temperature
Saturated Solution
69
If the solvent can’t dissolve the solute and need to be heated for it to be dissolved.
Supersaturated Solution
70
The relative amount of solute present in a solution.
Concentration of a solution

ChemTech (3 decks)

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