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Fundementals of Chem > Exam 1: Chapter 2 > Flashcards

Exam 1: Chapter 2 Flashcards

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1
Q

What does v stand for?

A

Frequency

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2
Q

What does λ stand for?

A

Wavelength

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3
Q

What does c stand for?

A

Speed of light

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4
Q

What is the relationship between the ENERGY of a photon of light and its FREQUENCY

A

Energy and frequency are directly proportional

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5
Q

What is the relationship between the ENERGY of a photon of light and its WAVELENGTH λ?

A

Energy and wavelength are inversely proportional

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6
Q

E=hv= h x c/ λ

A

Energy = Planck’s constant x frequency = Planck’s constant x speed of light / wavelength

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7
Q

What does “n” stand for?

A

Shell number or energy level number

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8
Q

What is the ground state?

A

The lowest energy (n=1)

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9
Q

What is the quantum theory big idea 1?

A

wave-particle duality: light has the characteristics of both waves and particles based on perspective

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10
Q

What is the quantum theory big idea 2?

A

Physical properties can be associated with electron waves

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11
Q

What does the principal quantum number (n) describe?

A

The energy level or shell

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12
Q

What does the angular momentum number (l) describe?

A

The “shape” or sub-shell

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13
Q

Equation to calculate energy of nth level of an electron

A

En = -2.178 x 10^-18J (1/n^2)

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14
Q

What is the shape of the 1s orbital

A

-Spherical shape
-n=1 radial nodes

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15
Q

What is the shape of the 2p orbital?

A

-dumbbell
- 1 angular node

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16
Q

What is the shape of the 3D orbital?

A

-more lobes
-2 angular nodes

17
Q

What is the Pauli exclusion principle?

A

Each electron in an atom is uniquely labeled by four quantum energy numbers

18
Q

What is the aufbau principle?

A

Building multi-electron atoms

19
Q

What are the rules of the aufbau principle?

A

1) Lower energy orbitals fill before higher energy orbitals
2) an orbital can hold a max of two electrons; both must have opposite spins
3) If two or more orbitals of of equal energy are available follow Hund’s rule

20
Q

What is Hund’s rule?

A

When filling orbitals with equal energy, fill the orbitals with single electrons before pairing electrons

Fundementals of Chem (5 decks)

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