Chemistry Ch. 4
What is not a possible value for n?
(-infinity, 0]
What values can the angular momentum quantum number have when n= 2
0,1
How many orientations can an s orbital have about the nucleus?
1
The set of orbital that are dumbbell shaped and directed along the x.y, and z axes are called
p orbitals
The number of sublevels within each energy level of an atom is equal to the value of the
principal quantum number
The main energy levels of an atom are indicated by the
principal quantum numbers
The letter designations for the first four sublevels with the max number of electrons that can be accommodated in each sublevel are
s:2, p:6, d:10, f:14
A 3-D region about the nucleus with a 95% probability of finding an electron
Orbital
The number of orbitals for the d sublevel is
5
The p sublevel may have a max of how many electrons
6
For the f sublevel the number of orbitals is
7
How many f orbitals make up the f sublevel
7
Light can also be called what two things
electromagnetic radiation, EMR
The region outside the nucleus where an electron can most probably be found is the
electron cloud
Both the Heisenberg uncertainty principle and the Schrodiinger wave equation
led to the concept of atomic orbitals
Each atomic orbital is described by its principal quantum number followed by the
letter of the sublevel
A single piece of light
photon
A spherical electron cloud surrounding an atomic nucleus would best represent an
s orbital
The angular momentum quantum number indicates the
shape of an orbital
The major difference between a 1s orbital and a 2s orbital is that
the 2s orbital is at a higher energy level
The statement that electrons fill the lowest available energy orbital first is known as
the Aufbau principle
The statement that no two electrons in the same atom can have the same four quantum numbers, or stated another way, electrons in the same orbital must have opposite spin is known as
the Pauli exclusion principle
Which model of the atom explains the orbitals of electrons as waves?
the quantum model
Frequency=
waves/second ; Nu, v
"Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron and all electrons in singly occupied orbitals must have the same spin" is a statement of
Hund's rule
The f sublevel may have a max of how many electrons
14
What is the order in which electrons fill?
1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s
A single orbiital in the 3d level can hold ___ electrons
2
At n=1, the total number of electrons that could be found is
2
How many p orbitals make up the p sublevel
3
An orbital that can never exist according to the quantum description of the atom is
3f
How many quantum numbers are needed to describe the energy state of an electron in an atom?
4
According to the quantum theory of an atom, in an orbital
an electron's position cannot be known precisely
How fast does EMR travel?
at the speed of light (C)
All of the following describe the Heisenberg uncertainty principle except a) states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle b) it is one of the fundamental principles of our present understanding of light and matter c) helped lay the foundation for the modern quantum theory d) helps to locate an electron in an atom
d) helps to locate an electron in an atom
All of the following describe the Schrodinger wave equation except a) it is an equation that treats electrons in atoms as waves b) only waves of specific energies and frequencies provide solutions to the equation c) helped lay the foundation for the modern quantum theory d) similar to Bohr's theory
d) similar to Bohr's theory
How many electrons can occupy the s orbitals at each energy level?
two if they have opposite spins
