Chemistry-Chapter 2

Which scientist identified the nucleus of the atom

Ernest Rutherford

Electromagnetic (EM) radiation is measured in waves/seconds or?

Hertz (Hz)

When comparing two frequencies of EM radiation, the higher frequency has a _____ wavelength and the lower frequency has a _____ wavelength

Shorter

Longer

A _____ is the distance between two successive crests or troughs of adjacent waves

wavelength

A quantum of EM (light) energy is referred to as a______ and is released resulting in a distinct color

Photon

A ____ spectrum is produced when a electron moves from a _____ energy level to a _____ energy level

line

Higher

lower

When an electron changes from the ground state to the excited state energy is _____

Absorbed

When an electron changes from the excited state to the ground state energy is _____

released

If electrons in an atom have the lowest possible energies, the atom is in the ____ state

ground

The _____ ______ is the region outside of the nucleus where an electron is likely found

electron cloud

What is the three-dimensional region around the nucleus called?

Orbital

Quantum theory stated that in an orbital an electrons positions ____ be known precisely

CANNOT

How many quantum numbers are used to describe the energy state of an electron?

4 (n, L, ML, MS)

The name of the quantum number that describes the main energy level is the?

Principle energy level

The shape of an orbital is indicated by the _____ _______ quantum number

Angular Momentum

What values can the angular momentum quantum number have when

n=1

n=2

n=3

n=4

1. 0

2. 0,1

3. 0,1,2

4.

How many spin states are here for an electron in an orbital which are indicated by the spin quantum #?

2

What is the shape of the s orbital

What is the shape of the p orbital

Spherical

Dumbell

What is the major difference between 1s and 2s orbitals

2s is higher energy level and is larger than 1s

What are the major differences between 2s and sp orbitals

2s is spherical

2p is dumbbell shaped + is higher energy level

What are the maximum number of electrons that can be accommodated in each of the four sublevels

s=2

p=6

d=10

f=14

How many orbitals does each sublevel have?

s=1

p=3

d=5

f=7

How many orientations can each sublevel have?

s=1

p=3

d=5

f=7

if n is the principle number of a main energy level, what algebraic expression to determine the number of electrons in that energy level?

2n²

How many electrons can completely fill the first energy level? second? third? fourth?

first:2

Second:8

Third:18

Four:32

a single orbital in any sublevel can hold _ electrons

2

If the second energy level already has 6 electrons how many are needed to fill it?

2

If the third energy level already has 10 electrons how many are needed to fill it?

8

What states that an electron occupies the lowest available energy level orbital and it specifies the sequence or order in which energy sublevels are filled

Aufbau Principle

what states that no two electrons can have the same for quantum numbers and that 2 electrons in the same orbital must have opposite spin?

Pauli exclusion principle

What requires that each of the orbitals at a particular energy level receive once electron before any of them can have two electrons (or before electrons begin pairing up)

Hunds rule