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MCAT General Chemistry > Chapter 1 > Flashcards

Chapter 1 Flashcards

1
Q

Protons

A
  • found in nucleus
  • charge = 1.6*10^-19 OR +1
  • Mass of 1 amu (atomic mass unit)
  • Elements are defined by their # of protons
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2
Q

The atomic number (Z) is equal to

A

the number of protons found in an atom of that element

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3
Q

Neutrons

A
  • Have no charge
  • Found in nucleus with protons
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4
Q

Mass number

A

Sum of protons and neutrons in nucleus

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5
Q

Isotopes

A
  • Share atomic # but different mass #s
  • Only differ in number of neutrons, same amount of protons
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6
Q

Electrons

A
  • Found in orbitals around nucleus
  • Charge of -1
  • Electrons closer to nucleus have lower energy
  • Electrons farther from nucleus (higher shells) have more energy
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7
Q

Valence electrons

A

Electrons farthest from nucleus that have strongest interaction with surroundings and weakest interactions with nucleus
* Most likely to bond with other atoms due to weak pull from own nucleus
* Determine reactivity

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8
Q

Losing electrons yields

A

positive charge

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9
Q

Gaining electrons yields

A

negative charge

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10
Q

Positively chargted atom

A

Cation

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11
Q

Negatively charged atom

A

Anion

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12
Q

Atomic Mass

A

Nearly equal to mass number (sum of protons and neutrons)
Think mass … mass number

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13
Q

Atomic Weight

A
  • Weighted average of all the different isotopes making up an element
  • Number found on the periodic table
    Think weight … weighted average
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14
Q

Mole

A
  • Can be atoms, ions, molecules, etc.
  • =6.02*10^23
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15
Q

Planck Relation

A
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16
Q

Planck’s constant

A

h=6.626*10^-34

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17
Q

Angular Momentum

A

h = Planck’s constant
n = principal quantum number

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18
Q

Energy of an electron

A
  • Changes in discrete amounts with respect to the quantum number
  • Energy of an electron increases (become less negative) the farther it is from the nucleus

R_H is the Rydberg unit of energy

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19
Q

Ground State

A
  • State of lowest energy
  • All electrons are in lowest possible obirtals
  • Desire this minimal energy state
20
Q

Excited State

A
  • Electron is promoted to an orbit with a larger radius (higher energy)
  • At least one electron has moved to a subshell with higher than normal energy
  • Will occur due to extremely high temperatures or irradation
21
Q

Electron movement from low to high energy

A

AHED
A Absorb light
H Higher potential
E Excited
D Distant (from nucleus)

22
Q

Electromagnetic Energy of photons

A
23
Q

Line spectrum

A

Emission spectrum with each line corresponding to a specific electron transition

24
Q
A

Energy of emitted photon corresponds to difference in energy between the initial state (higher energy) and the final state (lower energy)
+E = emission
-E = absorption
To gain energy, must absorb energy from photons too jump up to higher energy level

25
Q

Maximum number of electrons within a shell

A

2n^2

26
Q

Principal Quantum Number (n)

A
  • The larger the value of n, the higher the energy level and radius of the electron’s shell
  • Difference in energy between two shells descreases as distance from nucleus increases
27
Q

Azimuthal (Angular Momentum) Quantum Number (l)

A
  • Shape and number of subshells within a given principal energy level (shell)
  • l = 0 to (n-1)
28
Q

Subshells

A

l=0 (s)
l=1 (p)
l=2 (d)
l=3 (f)

29
Q

Maximum number of electrons within a subshell

A

4l+2

30
Q

Magnetic quantum number (m_l)

A
  • Specifies the orbital within a subshell where an electron will be most likely found at a certain time
  • Each orbital can hold max 2 electrons
  • Possible values: - l, 0, +l
31
Q

Orbital Shapes

A
32
Q

Subshell Amounts

A

S: 1 (2 elements)
P: 3 (6 elements)
D: 5 (10 elements)
F: 7 (14 elements)

33
Q

Spin quantum number (m_s)

A
  • When two electrons are in the same orbital, they must have opposite spins (AKA being paired)
  • Electrons in different orbitals with the same m_s have parallel spins
34
Q

____ will fill first

A

Subshells with lower energy

35
Q

n + l Rule

A

Lower n+l value has lower energy, therefore filling first

36
Q

Electron Configuration

A
37
Q

Electron Configuration of Ions

A

Will remove from subshell with higher principal quantum number first, then go down

38
Q

Half-filled and fully filled orbitals have …

A

lower energy and higher stability

39
Q

TWO Electron Configuratoin Exceptions

A

Chromium: [Ar]4s^1 3d^5
* Half fills 3d subshell making a lot more stable

Copper: [Ar] 4s^1 3d^10
* Fully fills 3d subshell making a lot more stable

Other elements in this group exhibit the same behavior
Similar shifts seen in f subshell but NEVER p subshell

40
Q

Paramagnetic

A

Materials made of atoms with unpaired electrons will orient their spins with the magnetic field, thus the material will be weakly attracted to the magnetic field

41
Q

Diamagnetic

A

Materials made of atoms with paried electrons, thus the material will be slightly repelled by a magnetic field

42
Q

Heisenberg Uncertainty Principle

A

It is impossible to determine at the same time with perfect accuracy the momentum and position of an electron

43
Q

Hund’s Rule

A

Orbitals are filled so there are a maximum number of half-filled orbitals with parallel spins

44
Q

Parallel

A

Electrons in different orbitals with the same m_s

45
Q

Speed of light in a vacuum (C)

A

3*10^8

MCAT General Chemistry (12 decks)

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