Chapter 1.1: Electronic Structure of Atoms

Question 1

What is the spreading of electron density over a large volume of space?

Answer 1

delocalization

Question 2

Define valence electrons

Answer 2

electrons in the valence (outermost) shell of an atom

Question 3

Define ionization potential

Answer 3

the energy needed to remove the most loosely held electron from an atom or molecule

Question 4

What is the outermost occupied electron shell of an atom?

Answer 4

valence shell

Question 5

Define orthogonal

Answer 5

having no net overlap

Question 6

What is the symbol of an element surrounded by a number of dots equal to the number of electrons in the valence shell of the atom?

Answer 6

Lewis Dot Structure

Question 7

What is the ability to do work?

Answer 7

energy

Question 8

What does Hund’s Rule state?

Answer 8

• Hund’s Rule states that when orbitals of equal energy are available but there are not enough electrons to fill all of them completely, one electron is put in each before a second electron is added to any

Question 9

What states that when orbitals of equal energy are available but there are not enough electrons to fill all of them completely, one electron is put in each before a second electron is added to any?

Answer 9

Hund’s Rule

Question 10

Define quantization

Answer 10

having specific values for energy and momentum

Question 11

Define shells

Answer 11

a region of space around a nucleus that can be occupied by electrons, corresponding to a principle quantum number

Question 12

Define energy

Answer 12

the ability to do work

Question 13

What does the Pauli Exlusion Principle state?

Answer 13

• The Pauli Exclusion Principle states that no more than two electrons may be present in an orbital. If two electrons are present, their spins must be paired

Question 14

What does an atom consist of?

Answer 14

• An atom contains a small, dense nucleus made of neutrons and positively charged protons
o Nucleus surrounded by negatively charged electrons

Question 15

Define delocalization

Answer 15

the spreading of electron density over a large volume of space

Question 16

What is the energy that can be released if given an opportunity?

Answer 16

potential energy

Question 17

Define Ground-State Electron Configuration

Answer 17

the lowest energy electron configuration of an atom or molecule

Question 18

Define excited state

Answer 18

a state of a system at higher energy than the ground state

Question 19

What are electrons in the valence (outermost) shell of an atom?

Answer 19

valence electrons

Question 20

Define ground state

Answer 20

the lowest energy state of a system

Question 21

What is Golden Rule #1?

Answer 21

o Golden Rule #1: In most stable molecules, the atoms have filled valence shells

Question 22

What is having no net overlap?

Answer 22

orthogonal

Question 23

What does the Aufbau Principle state?

Answer 23

• The Aufbau Principle states that orbitals fill in order of increasing energy, from lowest to highest

Question 24

What is the energy needed to remove the most loosely held electron from an atom or molecule?

Answer 24

ionization potential

Question 25

Define Lewis Dot Structure

Answer 25

the symbol of an element surrounded by a number of dots equal to the number of electrons in the valence shell of the atom

Question 26

What states that no more than two electrons may be present in an orbital. If two electrons are present, their spins must be paired?

Answer 26

The Pauli Exclusion Principle

Question 27

What is a region of space that can hold two electrons?

Answer 27

orbital

Question 28

What is the lowest energy state of a system?

Answer 28

ground state

Question 29

What is having specific values for energy and momentum?

Answer 29

quantization

Question 30

What is a region of space around a nucleus that can be occupied by electrons, corresponding to a principle quantum number?

Answer 30

shells

Question 31

Define potential energy

Answer 31

the energy that can be released if given an opportunity

Question 32

What is a state of a system at higher energy than the ground state?

Answer 32

excited state

Question 33

How many electrons can each shell hold?

Answer 33

2n^2, where n is the number of the shell

Question 34

What is the most important question in Organic Chemistry?

Answer 34

Where are the Electrons?

Question 35

What are the 3 rules the determine the ground-state electron configuration?

Answer 35

1. The Aufbau Principle
2. The Pauli Exclusion Principle
3. Hund’s Rule

Question 36

What states that orbitals fill in order of increasing energy, from lowest to highest?

Answer 36

The Aufbau Principle

Question 37

What is the lowest energy electron configuration of an atom or molecule?

Answer 37

ground-state electron configuration

Question 38

What is the relationship between shell number of electron energy?

Answer 38

 Higher shell number = more electron energy

Question 39

What are the 3 effects of quantized electron energy?

Answer 39

• 3 effects: electrostatic attraction that draws the electrons toward the nucleus; electrostatic repulsion between the electrons; wavelike nature of an electron that prefers to be delocalized, thereby spreading the electron density away from the nuclei

Question 40

Define valence shell

Answer 40

the outermost occupied electron shell of an atom

Question 41

Define orbital

Answer 41

a region of space that can hold two electrons