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Chemistry 1100 > Chapter 7 Definitions > Flashcards

Chapter 7 Definitions Flashcards

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1
Q

Quantum Mechanics

A

The theory that explains the behavior of the absolutely small

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2
Q

Waves out of phase means destructive Interference. True/False

A

True

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3
Q

Waves in phase means constructive Interference. True/False

A

True

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4
Q

Waves out of phase make bright spot. True/False

A

Dark Spot

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5
Q

Waves in phase makes bright spot. True/False

A

True

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6
Q

What are photons?

A

Discrete packets of light

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7
Q

What do prisms do?

A

They separate component wavelengths.

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8
Q

Light is emitted as electron falls back to a lower energy lever. True/False

A

True

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9
Q

Quantum-Mechanical Model

A

Explains how electrons exist in atoms and how the electrons determine the chemical and physical properties of elements

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10
Q

Electric Field

A

A region of space where an electrically charged particle experiences a force

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11
Q

Magnetic Field

A

A region of space where a magnetic particle experiences a force.

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12
Q

Amplitude

A

Vertical height. The amplitude determines the light’s intensity or brightness. Greater the amplitude, the greater the brightness

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13
Q

Wavelength

A

Distance between waves. Greater the wavelength, less frequency. Different wavelengths means different colors. Longer wavelengths means red (low energy). Shorter wavelengths means violet (high energy).

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14
Q

List the electromagnetic spectrum from low energy to high energy?

A

Radia, Microwaves, Infrared, Visible Light. Ultraviolet, X-ray, Gamma ray

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15
Q

Our eyes can only see reflected light. True/False

A

True

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16
Q

What is on the right side of the electromagnetic spectrum

A

High energy, short wavelength, and high frequency

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17
Q

What is on the left side of the electromagnetic radiation?

A

Low energy, Long wavelength, and low frequency

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18
Q

Interference

A

How waves interact with each other

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19
Q

The photoelectric effect

A

Observation that metals can emit electrons when light shines upon them

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20
Q

Atomic spectroscopy

A

The study of the electromagnetic radiation and emitted by atoms

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21
Q

Emission Spectrum

A

A series of bright lines at specific wavelengths

22
Q

The white light spectrum is continuous? True/False

A

True. It consists of light of all wavelength

23
Q

De Broglie Relation

A

The wavelength of an electron mass moving at velocity

24
Q

Probability distribution map

A

Shows where an electron is likely to be found

25
Q

Indeterminacy (vague)

A

Position of an electron is not possible

26
Q

The solution to the Schrodinger equation for an atom results in three quantum numbers. True/False

A

True. These numbers describe the size, energy, shape, and orientation of orbitals or energy levels. These are for hydrogen atoms.

27
Q

What is the Principal Quantum Number (n)

A

An integer that determines the overall size of the orbital and indicates the energy level of an electron in an orbital

28
Q

Angular Momentum Quantum Number (azimuthal quantum number)(l)

A

An integer that relates with the shape of the orbital

29
Q

Magnetic Quantum Number(ML)

A

An integer that specifies the orientation of the orbital

30
Q

What is orbital with same principal level

A

This means that orbitals have the same value of n

31
Q

What is orbital with same sublevel(subshell)

A

This means the orbitals have the same value of n and l

32
Q

Probability Density

A

The probability(per unit volume) of finding the electron at a point in space. As you move away from the nucleus the probability density decreases.

33
Q

Radial Distribution Function

A

Total probability of finding the electron within a thin spherical shell at a distance r from the nucleus. It has a value of zero at the nucleus.

34
Q

Node

A

Point where the wave function and the probability density and radial distribution all go through zero. The probability of finding an electron at a node is zero. It separates the phases of an orbital

35
Q

Two types of nodes

A

Angular and radial

36
Q

Radial Nodes (spherical node)

A

Spherical surface region where the probability of finding an electron is zero

37
Q

Angular Nodes

A

Always equal to the angular momentum Quantum Number. For an s orbital there are no angular nodes. These are planes or surfaces where there is a zero probability of finding an electron

38
Q

Phase

A

The sign of the amplitude of a wave(positive or negative). Important in bonding

39
Q

Electron Configuration

A

Indicates what orbitals are occupied by electron

40
Q

Ground State

A

Lowest energy electron configuration

41
Q

Electron Spin (Stern-Gerlach Experiment)

A

The direction of the arrow in an orbital diagram (pointing up or down)

42
Q

Spin Quantum Number (Ms)

A

The spin of an electron is specified by a fourth quantum number

43
Q

Pauli Exclusion Principle

A

No two electron in an atom can have the same four quantum numbers. Implies that each orbital can have a maximum of only two electrons, with opposing spins

44
Q

Coulombs Law

A

The interactions between charged particles

45
Q

Shielding

A

How one electron can shield another electron from the full charge of the nucleus

46
Q

Penetration

A

how one atomic orbital can overlap spatially with another, thus penetrating into a region close to the nucleus.

47
Q

Aufbau Principle (build up)

A

An electron occupies orbitals in order form lowest energy to highest

48
Q

Hund’s Rule

A

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

49
Q

Paramagnetic

A

An atom or ion that contains unpaired electrons is attracted to an external magnetic field

50
Q

Diamagnetic

A

Chemistry 1100 (3 decks)

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