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Chemistry 107 > Exam 4 > Flashcards

Exam 4 Flashcards

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1
Q

Defined as one-half the distance between the centers of two adjacent atoms

A

Metallic radius

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2
Q

Defined as one-half the distance between the centers of the atoms in the molecules

A

Covalent radius

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3
Q

The minimum energy(kJ/mol) required to remove sn electron from a gaseous atom in its ground state

A

Ionization energy

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4
Q

The negative of the energy change that occurs when an electron is accepted by an atom in the gaseous state to form an anion

A

Electron affinity

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5
Q

X + e = X-

A

Electron affinity

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6
Q

Have the same number of electrons, and hence the same ground-state electron configuration
Ex. Na+, Al3+, F-, O2-, and N3-

A

Isoelectronic

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7
Q

The positive charge felt by an electron

A

Effective nuclear charge(Zeff)

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8
Q

The outer shell electrons of an atom. Participate in chemical bonding

A

Valence electrons

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9
Q

The electrostatic force that holds ions together in an ionic compound

A

Ionic bond

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10
Q

The energy required to completely separate one mole of a solid ionic compound into gaseous ions

A

Lattice energy

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11
Q

A chemical bond in which two or more electrons are shared by two atoms

A

Covalent bond

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12
Q

Two atoms share two pairs of electrons

A

Double bond

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13
Q

Two atoms share three pairs of electrons

A

Triple bond

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14
Q

A covalent bond with greater electron density around one of the two atoms

A

Polar covalent bond or polar bond

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15
Q

The ability of an atom to attract toward itself the electrons in a chemical bond

A

Electronegativity

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16
Q

The difference between the number of valence electrons in an isolated atom and the number of electrons assigned to that atom in a leeis structure

A

Formal charge

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17
Q

One of two or more lewis structures for a single molecule that cannot be represented accurately by only one lewis structure

A

Resonance structure

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18
Q

The enthalpy change required to break a particular bond in one mole of gaseous molecules

A

Bond enthalpy

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19
Q

The distance between identical points on successive waves

A

Wavelength

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20
Q

The vertical distance from the midline of a wave to the peak or trough

A

Amplitude

21
Q

The number of waves that pass through a particular point in 1 second

A

Frequency

22
Q

The interaction between waves

A

Interference

23
Q

Waves that interact so that they add to make a larger wave are said to be in phase

A

Constructive interference

24
Q

Waves that interact so that they cancel each other are said to be out of phase

A

Destructive interference

25
Q

n-l-1

A

Equation to find nodes

26
Q

Represents the total probability at a certain distance from the nucleus

A

Radial distribution function

27
Q

Principle quantum number(energy level)

A

n

28
Q

Angular momentum quantum number(orbital type)

A

l

29
Q

Magnetic quantum number(position of orbital)

A

ml

30
Q

Spin quantum number(orientation of the spin)

A

ms

31
Q

The more accurately you know the position of a small particle, such as an electron, the less you know about its speed(momentum), and vice versa

A

heisenberg’s uncertainty principle

32
Q

Allows us to calculate the probability of finding an electron with a particular amount of energy at a particular location in the atom

A

Schrodinger’s equation

33
Q

A probability distribution map of a region where the electron is likely to be found

A

Orbital

34
Q

Represents the total probability of finding an electron at a particular point in space

A

Probability density function

35
Q

Same sign

A

Phase

36
Q

Opposite signs

A

Out of phase

37
Q

The sign of the wave function

A

Phase

38
Q

Distance of electrons from the nucleus

A

n

39
Q

Spherical

A

S orbitals

40
Q

Like two balloons tied at the knots(dumbbell shape)

A

P orbital

41
Q

Like four balloons toed at the knots

A

D orbital

42
Q

Like eight balloons tied at the knots

A

F orbital

43
Q

Shape of the volume of space that electron occupies

A

l

44
Q

Orientation of the orbital in space

A

ml

45
Q

No two electrons in an atom can have the same four quantum numbers

A

Pauli exclusion principle

46
Q

Fill-up electrons in lowest energy orbitals

A

Aufbau principle

47
Q

The most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins

A

Hund’s rule

48
Q

Unpaired electrons

A

Paramagnetic

49
Q

All electrons paired

A

Diamagnetic

Chemistry 107 (1 decks)

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