GenChem Exam 1 (Original)

Number of wave cycles (peaks or troughs) that pass a specified point in space per unit time; inversely proportional to wavelength.

Frequency(v)

Distance between two consecutive peaks or troughs in a wave; inversely proportional to frequency

Wavelength(λ)

0 lone pairs, 2 bonds

Shape, Angle, and Hybridization?

Linear, 180, sp

0 lone pairs, 3 bonds

Shape, Angle, and Hybridization?

Trigonal planar, 120, sp²

1 lone pair, 2 bonds

Shape, Angle, and Hybridization?

Bent/angular, <120, sp²

0 lone pairs, 4 bonds

Shape, Angle, and Hybridization?

Tetrahedral, 109, sp³

1 lone pair, 3 bonds

Shape, Angle, and Hybridization?

Trigonal pyramid, <109, sp³

2 lone pairs, 2 bonds

Shape, Angle, and Hybridization?

Bent/angular, <109, sp³

0 lone pairs, 5 bonds

Shape and Angle?

Trigonal bipyramid, 90 and 120

1 lone pair, 4 bonds

Shape and Angle?

Seesaw, <90 and <120

2 lone pairs, 3 bonds

Shape and Angle?

T-shape, <90

3 lone pairs, 2 bonds

Shape and Angle?

Linear, 180

0 lone pairs, 6 bonds

Shape and Angle?

Octahedral, 90

1 lone pair, 5 bonds

Shape and Angle?

Square pyramid, <90

2 lone pairs, 4 bonds

Shape and Angle?

Square planar, 90

3 lone pairs, 3 bonds

Shape and Angle?

T-shape, <90

4 lone pairs, 2 bonds

Shape and Angle?

Linear, 180

Orbitals that have the same energy.

Degenerate orbitals

Spherical region of space with high electron density; describes orbitals with l = 0.

s orbital

Dumbbell-shaped region of space with high electron density; describes orbitals with l = 1.

p orbital

Region of space with high electron density that is either four lobed or contains a dumbbell and torus shape; describes orbitals with l = 2.

d-orbital

Multi-lobed region of space with high electron density; describes orbitals with l = 3.

f orbital

State in which the electrons in an atom, ion, or molecule have the lowest energy possible.

Ground state

Rule stating that it is impossible to exactly determine both momentum and the position of a particle at the same time. The uncertainty principle is a consequence of quantum particles exhibiting wave–particle duality.

Heisenberg uncertainty principle

Every orbital in a sub-shell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Hund’s rule

Specifies that no two electrons in an atom can have the same value for all four quantum numbers.

Pauli exclusion principle

Quantum number specifying the shell an electron occupies in an atom.

Principle quantum number(n)

Quantum number distinguishing the different shapes of orbitals.

Angular momentum quantum number (l)

Quantum number signifying the orientation of an atomic orbital around the nucleus.

Magnetic Quantum Number (m_l)

Number specifying the electron spin direction, either +1/2 or −1/2.

Spin quantum number(m_s)

What bond is this?

Sigma bond

What bond is this?

Pi bond

Sigma_px Bond

Sigma_px Star Bond

Pi Bond

Pi_p Star Bond

List IMF’s from weakest to strongest.

London dispersion, Induced dipole-dipole, dipole-dipole, Hydrogen, Ion-dipole, Ion-ion

List IMF’s from strongest to weakest.

Ion-ion, Ion-dipole, Hydrogen, Dipole-dipole, Induced dipole-dipole, London dispersion

Model of the atom in which there is one electron.

Bohr Model

What is this formula?

Valence electrons-(number of bonds+lone pairs)

Formal Charge

As bonds degree increases they get?

Shorter