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ChemTech > GenChem_ARC > Flashcards

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
Q

Atomic Number

A

Number of protons in nucleus.

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26
Q

Mass Number (Atomic Mass)

A

Number of protons + neutrons.

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27
Q

Atoms of the same element with varying number of neutrons.

A

Isotopes

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28
Q

Carbon has three naturally occurring isotopes with ______ having the highest percent abundance.

A

C-12

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29
Q

He arranged the elements in groups of 3’s or triads also known as Law of Triad (1829).

A

Johann Wolfgang Dobereiner

30
Q

Arranged the elements in groups of 8’s or Law of Octaves (1894).

A

John Newlands

31
Q

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.

A

Julius Lothar Meyer

32
Q

He formulated the Periodic Law.

A

Dmitri Mendeleev

33
Q

The seven horizontal rows in the periodic table are called

A

PERIODS

34
Q

The vertical columns are called

A

GROUPS or FAMILIES

35
Q

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.

A

Noble Gases

36
Q

rare-earth elements

A

Lanthaniods

37
Q

heavy rare elements

A

Actinoids

38
Q

The average distance between nucleus and the valence electron.

A

Atomic Size (Atomic Radius)

39
Q

It is the ability of the atom to donate electrons.

A

Metallic Property

40
Q

Tendency of an atom to react.

A

Reactivity

41
Q

The amount of energy required to remove an electron from an atom or ion.

A

Ionization Energy

42
Q

The change in energy when an electron is accepted by a gaseous atom to form an anion.

A

Electron Affinity

43
Q

Defined as the relative ability of an atom of an element to attract or gain electrons.

A

Electronegativity

44
Q

The orbitals of an atom must be filled up in increasing energy levels.

A

Aufbau Principle

45
Q

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.

A

Pauli’s Exclusion Principle

46
Q

The most stable arrangement of electrons in subshells is the one with more parallel spins.

A

Hund’s Rule of Multiplicity

47
Q

The average distance of the electron from the nucleus in a particular orbital.

A

Principal Quantum Number

48
Q

It tells the shape of the orbital.

A

Azimuthal / Angular Momentum Quantum Number

49
Q

It describes the orientation of orbital.

A

Magnetic Quantum Number

50
Q

It shows the spin of electrons.

A

Spin Quantum Number (𝒎𝒔)

51
Q

The forces of attraction that hold together atoms or ions when they combine to form molecules or ion pairs in a given compound.

A

Chemical bonds

52
Q

An ionic bond is formed by actual electron-transfer; metal to non-metal.

A

Ionic Bonding

53
Q

It is formed by electron sharing; non-metal to non-metal.

A

Covalent Bonding

54
Q

One in which two or more substances (either elements or compounds) react to form one compound.

General Form: A + B  AB

A

Composition reaction

55
Q

One in which one compound decomposes to form two or more new substances.

General Form: AB  A + B

A

Decomposition reaction

56
Q

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

A

Single replacement reaction

57
Q

One wherein two compounds react to form two new compounds.

General Form: AX + BY  AY + BX

A

Double decomposition reaction

58
Q

substance that is oxidized

A

Reducing agent

59
Q

substance that is reduced

A

oxidizing agent

60
Q

The ratio of the total mass of each element to the total mass of one mole of the compound (MM) multiplied by 100%.

A

Percent Composition

61
Q

Gives the simplest ratio of the number of moles of atoms.

A

Empirical Formula

62
Q

Gives the actual ratio of the number of moles of atoms in a mole of the compound.

A

Molecular Formula

63
Q

Homogeneous mixture of 2 or more substances.

A

Solution

64
Q

dissolvingmedium

A

Solvent

65
Q

dissolve substance

A

Solute

66
Q

ability of a solvent to dissolve a salt at a particular temperature.

A

Solubility

67
Q

solvent can still dissolve the solute.

A

Unsaturated Solution

68
Q

if a solvent can’t no longer dissolve a given solute at a given temperature

A

Saturated Solution

69
Q

If the solvent can’t dissolve the solute and need to be heated for it to be dissolved.

A

Supersaturated Solution

70
Q

The relative amount of solute present in a solution.

A

Concentration of a solution

ChemTech (3 decks)

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