Flashcards in Exam 4 Deck (49)
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1
Defined as one-half the distance between the centers of two adjacent atoms
Metallic radius
2
Defined as one-half the distance between the centers of the atoms in the molecules
Covalent radius
3
The minimum energy(kJ/mol) required to remove sn electron from a gaseous atom in its ground state
Ionization energy
4
The negative of the energy change that occurs when an electron is accepted by an atom in the gaseous state to form an anion
Electron affinity
5
X + e = X-
Electron affinity
6
Have the same number of electrons, and hence the same ground-state electron configuration
Ex. Na+, Al3+, F-, O2-, and N3-
Isoelectronic
7
The positive charge felt by an electron
Effective nuclear charge(Zeff)
8
The outer shell electrons of an atom. Participate in chemical bonding
Valence electrons
9
The electrostatic force that holds ions together in an ionic compound
Ionic bond
10
The energy required to completely separate one mole of a solid ionic compound into gaseous ions
Lattice energy
11
A chemical bond in which two or more electrons are shared by two atoms
Covalent bond
12
Two atoms share two pairs of electrons
Double bond
13
Two atoms share three pairs of electrons
Triple bond
14
A covalent bond with greater electron density around one of the two atoms
Polar covalent bond or polar bond
15
The ability of an atom to attract toward itself the electrons in a chemical bond
Electronegativity
16
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
Formal charge
17
One of two or more lewis structures for a single molecule that cannot be represented accurately by only one lewis structure
Resonance structure
18
The enthalpy change required to break a particular bond in one mole of gaseous molecules
Bond enthalpy
19
The distance between identical points on successive waves
Wavelength
20
The vertical distance from the midline of a wave to the peak or trough
Amplitude
21
The number of waves that pass through a particular point in 1 second
Frequency
22
The interaction between waves
Interference
23
Waves that interact so that they add to make a larger wave are said to be in phase
Constructive interference
24
Waves that interact so that they cancel each other are said to be out of phase
Destructive interference
25
n-l-1
Equation to find nodes
26
Represents the total probability at a certain distance from the nucleus
Radial distribution function
27
Principle quantum number(energy level)
n
28
Angular momentum quantum number(orbital type)
l
29
Magnetic quantum number(position of orbital)
ml
30
Spin quantum number(orientation of the spin)
ms
31
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
heisenberg's uncertainty principle
32
Allows us to calculate the probability of finding an electron with a particular amount of energy at a particular location in the atom
Schrodinger's equation
33
A probability distribution map of a region where the electron is likely to be found
Orbital
34
Represents the total probability of finding an electron at a particular point in space
Probability density function
35
Same sign
Phase
36
Opposite signs
Out of phase
37
The sign of the wave function
Phase
38
Distance of electrons from the nucleus
n
39
Spherical
S orbitals
40
Like two balloons tied at the knots(dumbbell shape)
P orbital
41
Like four balloons toed at the knots
D orbital
42
Like eight balloons tied at the knots
F orbital
43
Shape of the volume of space that electron occupies
l
44
Orientation of the orbital in space
ml
45
No two electrons in an atom can have the same four quantum numbers
Pauli exclusion principle
46
Fill-up electrons in lowest energy orbitals
Aufbau principle
47
The most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins
Hund's rule
48
Unpaired electrons
Paramagnetic
49
