PRELIM 01 - Introduction to Organic Chemistry & Structure and Bonding Flashcards

1
Q

Is the chemistry of the compounds present in living organisms

A

Organic chemistry

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2
Q

The ability of atoms in forming stable bonds with itself

A

Catenation

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3
Q

Is defined as an atom or a group of atoms that effectively determines the chemical properties of an organic compound

A

Functional group

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4
Q

Is a series of compounds that have the same funcitonal group

A

Homologous series

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5
Q

Is the idea of an electron “orbiting” the nucleus like planets orbiting the sun

A

Orbit

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6
Q

Are electron clouds that represent the shape of probability for an electron’s location

A

Orbital

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7
Q

Tells about the detailed location of electrons in an atom and the specific electron orbitals that the electrons are found

A

Electron configuration

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8
Q

He is credited as the father of modern atomic theory

A

John Dalton

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9
Q

Proposed the planetary model of the atom

A

Niels Bohr

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10
Q

Principle that states that there is an inherent uncertainty in the act of measuring a variable of a particle

A

Heisenberg uncertainty principle

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11
Q

Atoms of the same element with different number of neutrons

A

Isotopes

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12
Q

Is weighted average mass in atomic mass units of an element’s naturally occuring isotopes

A

Atomic mass/Atomic weight

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13
Q

4 quantum numbers

A

Principal, Angular momentum, Magnetic, Spin

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14
Q

Orbital size and energy level (n)

A

Principal

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15
Q

Orbital shape (l)

A

Angular momentum

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16
Q

Orbital orientation (ml)

17
Q

Electron spin direction (ms)

18
Q

4 different kinds of orbitals for electrons

A

s, p, d, f

19
Q

Spherical; nucleus at the center

A

s orbitals

20
Q

Dumbbell-shaped; nucleus at middle

A

p orbitals

21
Q

Elongated dumbbell-shaped; nucleus at center

A

d orbitals

22
Q

Tetrahedral; nucleus at center

A

f orbitals

23
Q

Lobes of a p orbital are separated by region of zero electron density, which is called a __________

24
Q

Lowest energy arrangement of an atom

A

Ground-state electron configuration

25
Principle that states that lowest energy orbitals must be filled first
Aufbau 'build-up' principle
26
Principle that states that only two electrons can occupy an orbital, and they must be of opposite spin
Pauli exclusion principle
27
Principle that states that if two or more empty orbitals of equal energy are available, electrons occupy each with spins parallel until all orbitals have one electron
Hund's rule
28
Shows the valence electrons of atoms as dots
Lewis structures
29
Have a line drawn between two atoms indicating a covalent bond
Kekule structures
30
Valence electrons that are not used in bonding
Nonbonding electrons/Lone-pair electrons
31
Forms when two atoms approach each other closely so that a singly occupied orbital on one atom overlaps a singly occupied orbital on the other atom
Covalent bond
32
2 models to describe covalent bonding
Valence bond theory, Molecular orbital theory
33
Theory that states that electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms
Valence bond theory
34
Is where electrons are most likely to be found in a molecule
Molecular orbital
35
Theory that states that bonds results from combination of atomic orbitals to give molecular orbitals
Molecular orbital (MO) theory
36
Circular cross-section and are formed by head-on interaction
Sigma (σ) bond
37
"Dumbbell" shape from sideways interaction of p orbitals
Pi (π) bond