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MRII ChE Reviewer > Physical and Chemical Principles > Flashcards

Physical and Chemical Principles Flashcards

1
Q

Atomic Theory

A

John Dalton
1. Elements are composed of tiny indivisible particles called atoms. Atoms of different elements are chemically different; however, atoms of a given element are of the same size, shape, mass, and chemical properties.
2. Law of Multiple Proportions
3. Law of Conservation of Mass

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2
Q

If two elements combine to form more than one compound, the ratio of the mass of an element to a fixed mass of the other element is a whole number or a simple fraction.

A

Law of Multiple Proportions

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3
Q

A chemical reaction only involves separation, combination, or rearrangement of atoms.

A

Law of Conservation of Mass

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4
Q

A pure compound is made up of elements in the same proportion by mass.

A

Law of Definite Proportions

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5
Q

This scientist determined the charge of an electron to be -1.60 x 10^(-19) C.

A

Robert Andrews Millikan

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6
Q

This scientist determined the ratio of electric charge to the mass of an electron to be -1.76 x 10^(8) C/gram

A

Joseph John Thomson

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7
Q

These scientists discovered the Cathode Ray Tube

A

Sir William Crookes and Heinrich Geissler

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8
Q

This scientist discovered the X-rays, which penetrated matter, darkened unexposed photographic plates, and caused metals to emit unusual rays.

A

Wilhelm Konrad Rontgen

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9
Q

This scientist discovered radioactivity in uranium.

A

Antoine Henri Becquerel

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10
Q

This scientist discovered radioactivity in uranium and polonium. Also discovered radium.

A

Marya Skolodowska Curie

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11
Q

This scientist performed the gold foil experiment wherein a thin foil of gold was bombarded with alpha particles. He generalized that most of the atom is an empty space and that the positive charge of an atom is concentrated in the nucleus.

A

Ernest Rutherford

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12
Q

This scientist discovered neutron by bombarding a beryllium atom with alpha particles producing an electrically neutral particle having a mass slightly greater than that of a proton.

A

James Chadwick

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13
Q

What is the mass of a neutron?

A

1.67495 x 10^(-24) g

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14
Q

What is the mass of a proton?

A

1.67252 x 10^(-24) g

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15
Q

What is the mass of an electron?

A

9.1095 x 10^(-28) g

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16
Q

What are the respective charges of a proton and an electron?

A

1.6022 x 10^(-19) C and -1.6022 x 10^(-19) C

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17
Q

The number of protons in the nucleus of an atom.

A

Atomic number

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18
Q

The total number of protons and neutrons in the nucleus of an atom.

A

Mass number

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19
Q

Atoms that have the same atomic number but different mass number.

A

Isotopes

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20
Q

This quantum number pertains to the average distance of the electron from the nucleus in a particular orbital (has integral values 1, 2, etc.)

A

Principal Quantum Number (n)

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21
Q

This quantum number tells the shape of the orbital (has values from 0 to n-1)

A

Azimuthal/Angular Momentum Quantum Number (l)

22
Q

This quantum number describes the orientation of orbitals in space (allowable values from -l to 0 to +l)

A

Magnetic Quantum Number (m_l)

23
Q

This quantum number shows the spin of electrons (values +1/2 for clockwise and -1/2 for counter clockwise)

A

Spin Quantum Number (m_s)

24
Q

States that the orbitals of an atom must be filled up in increasing energy levels

A

Aufbau Principle

25
Q

States that 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 Exclusion Principle

26
Q

States that the most stable arrangement of electrons in subshells is the one with more parallel spins

A

Hund’s Rule of Multiplicity

27
Q

This scientist arranged the elements in triads like Li-Na-K, Ca-Sr-Ba, and Cl-Br-I.

A

Johann Wolfgang Dobereiner

28
Q

This scientist arranged the elements in atomic mass and found out that every eight element has similar properties.

A

John AR Newlands

29
Q

These scientists arranged the elements in the periodic table according to their recurring periodic properties.

A

Dmitri Ivanovich Mendeleev and Julius Lothar Meyer

30
Q

This scientist discovered the relationship between the elements’ atomic number and the frequency of X-rays generated by bombarding the element with high-energy electrons.

A

Henry Gwyn-Jeffreys Moseley

31
Q

This is the average distance between the nucleus and the valence electron.

A

Atomic Size (Atomic Radius)

32
Q

The energy required to remove an electron from a gaseous atom in its ground state. (The lower this is, the easier it is for an atom to form a cation)

A

Ionization Energy

33
Q

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

A

Electron Affinity

34
Q

The measure of the ability of an atom to attract towards itself a bonding electron.

A

Electronegativity

35
Q

This scientist is the recipient of the Nobel Prize in Chemistry in 1954 and the Nobel Peace Prize in 1962.

A

Linus Carl Pauling

36
Q

Trend of Atomic Size

A

Decreasing from Left to Right
Increasing from Top to Bottom

37
Q

Trend of Metallic Property

A

Decreasing from Left to Right
Increasing from Top to Bottom

38
Q

Trend of Reactivity

A

Decreasing from Left to Right
Increasing from Top to Bottom

39
Q

Trend of Electron Affinity

A

Increasing from Left to Right
Decreasing from Top to Bottom

40
Q

Trend of Electronegativity

A

Increasing from Left to Right”
Decreasing from Top to Bottom

41
Q

This is the bond formed from the attraction of the nucleus and the electron of two or more atoms and usually involves two non-metals.

A

Covalent Bond

42
Q

This is the bond formed from the attraction of two opposite charged particles and involves a metal and a non-metal.

A

Ionic Bond

43
Q

This pertains to single bond, double bond, or triple bond, and those intermediate between single and double bonds, etc.

A

Bond Order

44
Q

States that the formation of a bond is due to the overlap of two atomic orbitals

A

Valence Bond Theory

45
Q

States that a bond is formed when electrons in the bonding molecular orbital is greater than the electrons in the non-binding molecular orbital.

A

Molecular Orbital Theory

46
Q

With halogen displacement, what is the activity series?
Cl2 > Br2 > F2 > I2
I2 > Br2 > Cl2 > F2
F2 > Cl2 > Br2 > I2
F2 > Br2 > Cl2 > I2

A

F2 > Cl2 > Br2 > I2

47
Q

The total number of protons plus neutrons in the products and in the reactants must be the same.

A

Conservation of Mass Number

48
Q

The total number of nuclear charges in the products and in the reactants must be the same.

A

Conservation of Atomic Number

49
Q

Gibb’s Phase Rule

A

phases + deg. freedom = components + 2

50
Q
A
51
Q
A

MRII ChE Reviewer (1 decks)

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