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CCP 3 LEC > Atomic Structure > Flashcards

Atomic Structure Flashcards

2- Structure and Bonding

1
Q

subatomic particles found in the dense nucleus of an atom

A

protons and neutrons

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2
Q

surrounds the dense nucleus

A

electrons

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3
Q

most of the mass is in the _________

A

nucleus

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4
Q

most of the volume is in the _____

A

electron cloud

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5
Q

indicates the total number of protons and the number of neutrons present in an atom

A

mass number

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6
Q

states the number of protons present in an atom

A

atomic number

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7
Q

atoms with the SAME number of protons but DIFFERENT numbers of neutrons

A

isotopes

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8
Q

almost 99% of the carbon found in nature

A

12C

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9
Q

the exact location of the electron
CANNOT be known; ONLY the electron density can be known

A

Quantum Mechanical Model

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10
Q

the probability that the electron will be in a certain region of space (orbital) at a given instant

A

electron density

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11
Q

Where do electrons move instead of circling around the nucleus in fixed orbits?

A

orbitals

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12
Q

each orbital has a characteristic _ and _.

A

shape, size (energy)

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13
Q

used to describe orbitals

A

Quantum Numbers

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14
Q

4 quantum numbers

A
  1. Principal
  2. Azimuthal/Angular Momentum
  3. Magnetic
  4. Electron Spin
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15
Q

symbol for Principal quantum number

A

n

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16
Q

symbol for Azimuthal/
Angular Momentum quantum number

A

l

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17
Q

symbol for Magnetic quantum number

A

m_l

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18
Q

symbol for Electron Spin quantum number

A

m_s

19
Q
  • indicates the main energy level or shell (size) of an electron in an atom
  • represents the average distance of the electron from the nucleus
A

Principal

20
Q

determines the shape (subshell) of the orbital

A

Azimuthal/
Angular Momentum

21
Q

specifies the orientation of the orbital in space

A

Magnetic

22
Q

describes the spin (direction) of an electron within an orbital

A

Electron Spin

23
Q

values can be any positive integer and indicates the energy level or shell where electrons are located

A

Principal

24
Q

ranges from 0 to (n-1) / s, p, d, f; corresponds to different sublevels within each principal energy level

A

Azimuthal/
Angular Momentum

25
Q

ranges from -l to +l and defines the number of orbitals present within a sublevel

A

Magnetic

26
Q

can have one of two possible values: +1/2 (spin up) or -1/2 (spin down).

A

Electron Spin

27
Q

number of orbitals and electrons in s-subshell

A

one orbital, 2 electrons

28
Q

number of orbitals and electrons in p-subshell

A

three orbitals, 6 electrons

29
Q

number of orbitals and electrons in d-subshell

A

five orbitals, 10 electrons

30
Q

number of orbitals and electrons in f-subshell

A

seven orbitals, 14 electrons

31
Q

shape of s orbital

A

spherical

32
Q

shape of p orbital

A

dumbbell

33
Q

shape of four of the five d orbitals

A

cloverleaf

34
Q

shape of the fifth d orbital

A

elongated dumbbell with a doughnut around its middle

35
Q

describes where electrons are located around the nucleus of an atom

A

Electron Configuration

36
Q

describes the orbitals occupied by the atom’s electrons when they are all in the available orbitals with the lowest energy

A

Ground-state electron configuration

37
Q
  • Electrons fill the lowest energy orbitals available before moving to higher energy orbitals.
  • This principle dictates the order in which electrons occupy atomic orbitals.
A

Aufbau Principle

38
Q
  • Electrons prefer to occupy degenerate orbitals (orbitals of the same energy) singly with parallel spins before pairing up.
  • This maximizes the total electron spin and stabilizes the atom.

This requires single occupancy before pairing.

A

Hund’s Rule

39
Q
  • No two electrons in a atom can have an identical set of four quantum numbers.
  • This means an orbital can hold a maximum of two electrons, and then the electrons must have opposite spins, +1/2 and -1/2.
A

Pauli Exclusion Principle

40
Q

This principle states that it is impossible to simultaneously know the exact position and momentum (or velocity) of a particle, such as an electron.

A

Heisenberg’s Uncertainty Principle

41
Q

electrons below the outermost shell

A

Core Electrons

42
Q

electrons in the outermost shell

A

Valence Electrons

43
Q
A

CCP 3 LEC (4 decks)

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