Chemistry 11 - Atomic theory

levesque chemistryyy

Relative charge of protons

1+

Relative charge of neutrons

0

Relative charge of electrons

1-

The two subatomic particles responsible for almost all of an atom’s mass are the _____ and _____

protons, neutrons

Most of the atom’s volume is actually ____ ______

empty space

When atoms of a particular element differ in the number of electrons they create

ions

When atoms of a particular element differ in the number of neutrons they create

isotopes

Aufbau principle

States that in the ground state of an atom/ion, electrons fill lower energy orbitals before higher energy ones

Hund’s rule

When filling orbitals, electrons will individually occupy each orbital before any orbital is doubly occupied, and all singly occupied orbitals will have the same spin

Pauli Exclusion Principle

No two electrons can occupy the same set of quantum numbers

The electrons must have opposite spin

Light is

Electromagnetic radiation (EMS)

White light is made up of ________

all the frequencies and wavelengths of visible light spectrum (colors through a prism)

Continuous spectrum

A complete range of colors (like a rainbow) with no missing parts

All electromagnetic waves travel at the same ________

speed (3.00 × 10⁸ m/s)

Electromagnetic waves differ in terms of their _______

wavelength

The number of waves that pass a particular point in one second is called the ____________

frequency

When atoms are _____ (when heated/applied voltage) → when they absorb energy

excited

When the electron falls back to its ________, it releases ________ appearing as a ___________

groundstate, energy, wavelength of light

What is a line emission spectrum

A line emission spectrum shows only specific wavelengths (colors) of light that are given off by excited atoms.

Line emission spectrums are NOT _________

continuous

Discrete electron energy levels are: ______

Discrete electron energy levels are the specific, fixed energy levels that electrons can occupy in an atom — they can’t be in between

What does it mean when electrons are quantized

The electron can only have certain specific energy values, not just any amount, no in between

What did the idea of quantization lead to

The bohr model

The color of light released (photon) corresponds to _________

The energy difference between two energy levels

Equation relating to speed, wavelength & frequency

c = fλ

The four atomic orbital types

s, d, p, f

How many max. electrons can the “s” sublevel hold

2

How many max. electrons can the “p” sublevel hold

6

How many max. electrons can the “d” sublevel hold

10

How many max. electrons can the “f” sublevel hold

14

Exception: The expected configuration of chromium is: [Ar] 4s² 3d⁴: In order for the atomic orbitals to be stable, the actual electron configuration is:

[Ar] 4s¹ 3d⁵

Exception: The expected configuration of chromium is: [Ar] 4s² 3d⁹ : In order for the atomic orbitals to be stable, the actual electron configuration is:

[Ar] 4s¹ 3d¹⁰

The general order of electron removal to form positive ions is:

p, s, d, f

Isotopes have (almost) the same ___________ because they have the same number of electrons

reactivity

Different mass # means they have __________ __________ __________

different physical properties

What is a mass spectrometer and how does it work

A scientific instrument used to identify atoms or molecules by measuring their mass and charge. It separates particles (ions) based on their mass-to-charge ratio (m/z) and helps determine what they are and how much of them there is

As you move across a period, the nuclear charge __________

increases

As you move across a period, the atomic radius __________

decreases (drawing the electrons closer to the nucleus)

As you go down a row, more _________ are added which _____ the atomic radius

shells/orbitals, increases

As you move across a period, the electronegativity _________

increases

What is electronegativity

How much an atom wants to pull electrons toward itself

As you move down a group, the electronegativity _________

decreases

What is ionization energy

Ionization energy is the amount of energy needed to remove an electron from an atom to make an ion

An atom’s electronegativity has an _________ relationship with its atomic radius

inversely

As you go across a period, the ionization energy ______

increases

As you go down a group, the ionization energy _______

decreases

Example: Which is larger, magnesium or calcium

Explain !

(My explanation)

As you move down a group, elements gain electron shells therefore increasing the atomic radius. Calcium is larger than magnesium.

Example: Which has a higher electronegativity, sodium or potassium

Explain !

(My explanation)

Sodium is in a higher group than potassium which means that its electrons are closer to the nucleus resulting in a stronger attraction of electrons.

Example: Which has lower ionization energy, boron or aluminum

(My explanation)

Aluminum can lose an electron easier because it has a larger atomic radius, meaning electrons are less tightly held. Its outer electron is also furthest from the nucleus. Therefore aluminum has lower ionization energy.

To solve for the effective nuclear charge, we use the formula Zeff = Z-S. What does Z and S stand for?

Z = # of protons

S = # core electrons

A cation has a ______ radius than its neutral atom because it ______ valence electrons

smaller, loses

An anion has a ______ radius than its neutral atom because it ______ valence electrons

larger, gains