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General Chemistry For Engineers > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

Define Atomic mass

A

the average mass of the naturally occurring isotopes of an element

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2
Q

Define atomic radius

A

the distance from the nucleus to the outermost occupied electron orbital in an atom

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3
Q

State Aufbau principle

A

the procedure for assigning electrons to shells, subshells, and orbitals in the order of increasing energy.

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4
Q

What is Azimuthal quantum number ?

A

the number designation (l) of an electron subshell.

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5
Q

What is a closed shell?

A

a valence shell in an atom that has the maximum number of electrons allowed by the Pauli Exclusion Principle.

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6
Q

What is electron affinity?

A

the amount of energy released when an electron is added to a neutral atom in the gas phase

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7
Q

What is electronegativity ?

A

a measure of the tendency of an atom to attract electrons from another atom in a chemical bond

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8
Q

What is electron configuration?

A
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9
Q

What is an excited state?

A

higher energy state of an atom arising from the absorption of energy and the transition of electrons to higher orbitals.

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10
Q

Define : Principal quantum number

A

the number designation (n) of an electron shell. Proton a positively charged particle present in all atomic nuclei.

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11
Q

What is meant by : quantized ?

A

a quantity that is restricted to certain allowed values

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12
Q

How many naturally occurring elements are there?

A

98

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13
Q

What three particles make up an atom and what are their charges?

A
  1. Proton > positively charged
  2. Neutron > unchanged
  3. Electron > negatively charged
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14
Q

Where is the majority of the mass of an atom located?

A

Nucleus

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15
Q

Where is the majority of the volume of an atom located?

A

Electrons in their orbitals

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16
Q

What is the atomic number of an atom equal to?

A

Number of protons in the nucleus

17
Q

What is the mass number of an atom equal to?

A

Number of protons + number of neutrons

18
Q

What are the atomic symbols of the following elements: (a) boron, (b) antimony, (c) silver, (d) tungsten, (e) astatine, (f) iron?

A

a. B
b. Sb
c. Ag
d. W
e. At
f. Fe

19
Q

What are the names of the following elements:(a) Cl , (b) Cu , (c) Au , (d) Tl , (e) Na , (f) Rn?

A

a. Chlorine
b. Copper
c. Gold
d. Thallium
e. Sodium
f. Radon

20
Q

What are isotopes?

A

Elements that have the same number of protons but different number of neutrons

21
Q

How atomic mass different from mass number?

A

Mass number is equal to the number of protons and neutrons in the nucleus of an atom
Atomic mass average mass of all naturally occurring isotopes

22
Q

What determines the chemistry of an atom?

A

It’s electrons

23
Q

What is meant by electrons being quantized?

A

The energy of electrons is being restricted to certain allowed values

24
Q

What is the quantum number that designates an electron shell? What is its letter designation?

A

Principle of quantum number (n)

25
Q

What is the quantum number that designates an electron subshell? What is its letter designation?

A

Azimuthal quantum number (l)

26
Q

What is the quantum number that designates the spatial orientation of an orbital? What is its letter designation?

A

Magnetic quantum number (m)

27
Q

What is the Pauli Exclusion Principle?

A

No two electrons can have the same four quantum numbers

28
Q

List the four quantum numbers, their letter designations, and their allowed values.

A
  1. Principle of quantum number ….(n) …. 0,1,2,3..
  2. Azimuthal quantum number …. (l) …. -1,0,1..
  3. Magnetic quantum number …. (m) …. +l , 0 ,-l
  4. Spin quantum number …. (s) …. -½ , + ½
29
Q

What is the ground state of an atom?

A

Electronic configuration with the lowest possible energy

30
Q

What creates an atomic excited state?

A

Absorption of energy causing an electron to move to a higher energy orbital

31
Q

What is released when an electron falls from a higher orbital to a lower one?

A

Energy inform of light

32
Q

What is the Aufbau principle?

A

Procedure of assigning electrons into shells , sub shells and orbitals in oder of increasing energy

33
Q

What is Hund’s Rule?

A

Electrons will occupy orbitals individually before occupying them in pairs

34
Q

List the electron subshells in the order of increasing energy.

A

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General Chemistry For Engineers (2 decks)

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