Chapter 1: Atomic Structure

Question 1

Subatomic Particles:

Answer 1

Three types are: protons, neutrons, & electrons.

Question 2

Protons:

Answer 2

This is found in the nucleus of an atom, has a mass of 1 atomic mass unit (amu), is positive, and is the same as the atomic number. • Aka Atomic Number. • Equals to the number of electrons.

Question 3

Neutrons:

Answer 3

This is found in the nucleus of an atom, is neutral, has no charge, and has a mass larger than a proton.

Question 4

Atomic Mass/Mass Number:

Answer 4

This is the sum of the protons and neutrons in the atom’s nucleus. • Constant for a given element, and is on the periodic table. • Example: Oxygen has 16

Question 5

Atomic Weight:

Answer 5

This is similar to the mass number, but includes isotopes. • It’s the weighted average of different isotopes.

Question 6

Isotopes:

Answer 6

This are atoms that share an atomic number but have different mass numbers.

Question 7

Electrons:

Answer 7

These move through spaces surrounding the nucleus, has an equal but negative charge to a proton, and has a mass of 1/2000 of a proton.

Question 8

Distance of electrons in the nucleus: Closer to the nucleus = Further from the nucleus =

Answer 8

• If the electron is closer to the nucleus, it has a low energy level. • But if they are further from the nucleus, then it has a high energy level.

Question 9

Valence Electrons:

Answer 9

Electrons that are furthest from the nucleus. § They have the strongest interactions with the surrounding environment and the weakest with the nucleus. § It can determine the reactivity of an atom. Are on the peroidic table. They are the group numbers. So Hydrogen, lithium and more are in group 1, they will have 1 valence electron. Oxygen, sulfur, etc are in group 16 and they will have 6 valence electrons.

Question 10

Cations: Anions:

Answer 10

Cations: Positively charged atom. Anions: Negatively charged atom.

Question 11

Avogadro’s Number:

Answer 11

Equal to a “mole”. It’s value is 6.02x10²³.

A mole is a number of things.

Question 12

Quantum Mechanical model:

Answer 12

Posits that electrons do not travel in defined orbit but rather are localized in orbitals.

Question 13

Orbitals:

Answer 13

This is a region of space around the nucleus defined by the probability of finding an electron in that region of space.

Question 14

Heisenberg uncertainty principle:

Answer 14

States that it is impossible to know both an electrons position and its momentum exactly at the same time.

Question 15

Four quantum numbers:

Answer 15

Includes:

Principal Quantum Number:

Azimuthal Quantum Number:

Magnetic Quantum Number

Spin Quantum Number:

Question 16

Principal Quantum Number: (n)

Answer 16

This quantum number describes the average energy of a shell.

Question 17

Azimuthal Quantum Number: (l);

Answer 17

This quantum number describes the subshells within a given principal energy level. (s,d,p,f)

Question 18

Magnetic Quantum Number: (Ml);

Answer 18

This quantum number specifies the particular orbital within a subshell where an electron is likely to be found at a given moment in time.

Question 19

Spin Quantum Number: (Ms);

Answer 19

This quantum number indicates the spin orientation of an electron in an orbital.

Question 20

Electron Configuration:

Answer 20

The measure of the ability of an atom to attract the electrons in a bond.

It uses spectroscopic notation, where the first number is the principle energy level, and the letter designates the subshell, and the superscript gives the number of electrons in that subshell.

Question 21

Hund’s Rule:

Answer 21

Electrons fill orbitals according to this rule.

It states that subshells with multiple orbitals (p,d, and f) fill electrons so that every orbital in a subshell gets one electron before any of them gets a second.

Question 22

Electron Configuration of Negatively Charged Ions (Anions):

Answer 22

These will have an additional electrons.

Example: F (Fluroine) This is up to 2p.

So fluroine will be: 1s²2s²2p⁵, but

F- = 1s²2s²2p⁶

Question 23

Electron Configuration of Positively charged ions (Cations):

Answer 23

In this, electrons will be removed from the subshells with the highest values for n first.

Example:

Zn (Zinc) = 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

but Zn2+ = 1s²2s²2p⁶3s²3p⁶4s⁰3d¹⁰

Question 24

What is the electron configuration of Magnesium (Mg)?

Answer 24

It is located in the 3S section. So it will be 1s²2s²2p⁶3s².