Test 5 Electrons

3 rules that govern where the electrons will settle

1. Aufbau Principle: electrons occupy the lowest energy levels first. 2. Pauli Exclusion Principle: Each orbital can hold 2 electrons and each must spin in OPPOSITE 3. Hund's Rule: Electrons occupy equal energy orbitals so that a maximum of unpaired electrons results. (Basically the electrons don't get paired with each other unless they absolutely have to)

How to do shorthand configuration

1. Find the closest noble gas to the atom (or ion) WITHOUT GOING OVER the number of electrons in the atom/ion (just pick the one right before your desired element) 2. Find where to resume by finding the next energy level 3. Resume the configuration until it's finished

Atom behavior explained by Bohr's Model

1. It tells us that electrons move in circular paths called orbits. 2. Bohr thought that electrons have fixed amounts of energy which places them in different energy levels 3. Electrons can move from one energy level to another by gaining or losing an exact amount of energy called quantum. 4. Energy levels are not equally spaced, but get closer together as they move farther away from the nucleus

No more than ___ electrons can be assigned to one orbital.

2

Negative ions have __ electrons, positive ions have ___ electrons

Gained, lost

What model did Erin Schrödinger make and what does it mean?

He made the quantum mechanical model. - shows that electrons do not move in an exact path, but do have specific energies - a fuzzy cloud exists in the densest places. These dense places have the highest probability of finding electrons

What principle explained why it's only possible to know the PROBABILITY of an electron being somewhere?

Heisenberg uncertainty principle

exceptions to the octet rule

If d and f can't be full, it is also good to be HALF full. Electrons that are not full are usually d⁴ and d⁹. To fix this, the atom will move an electron from the s layer (so that it goes from s² to s¹), and then move that electron to the d layer with a missing electron. That way, all the layers can be either full, or half filled.

Heisenberg Uncertainty Principle

It is impossible to know the velocity and position of an electron at the same time. The better we know one, the less we know the other.

The three ways to show electron configurations and what they mean

Longhand configuration- the ENTIRE configuration of the element starting at 1s. Orbital diagram- the diagram with the arrows showing the direction the electron spins in Shorthand configuration- show the noble gas that comes before the element and then finish the configuration.

Electrons will be located at the areas with the ___ energy and the ___ stability.

Lowest energy; most stability

The electrons that are gained/lost in an ion should only be added or removed from the ___

OUTERMOST layer

Difference between orbits and orbitals

Orbital- area where an object (electron) can occupy Orbit- path

Are electrons found in orbitals or orbits?

Orbitals

Octet rule

Outermost electrons are always s & p. The max number of valence electrons is 8

Niels Bohr Model name and what it means

Planetary/ Orbital Model It explains atom behavior

What do electrons do when returning to their normal level (ground state)?

They release their energy as light

Can we predict orbits?

We CANNOT. We can only predict the probability of finding an electron a certain distance from the nucleus

Orbital

a region of space where there is a high probability of finding an electron

Electrons are divided between ___ and ___ electrons

core, valence

When electrons absorb light they ___

jump to higher energy levels

principle quantum # is represented by the letter __. It denotes ___. Currently, n can be ___ because that covers all elements we know (rows on the periodic table)

n; it denotes the shell (energy level) in which the electron is located; #1 - #7

How do electrons spin?

opposite directions- one spins clockwise, while the other spins counterclockwise

4 shapes of Orbitals: their names, their shape, the # of orbitals, and the # of electrons it can hold.

s: spherical; 1 orbital; 2 electrons total p: dumbbell; 3 orbitals; 6 electrons total d: clover; 5 orbitals; 10 electrons total f: complex; 7 orbitals; 14 electrons total

What is atomic emission spectrum

the certain frequencies released by electrons while they're returning to ground state. - these frequencies are like a fingerprint of the element - different gasses give off different colors of "neon light"