## 29 terms · Section Review 4.2 and 4.3

###
The letter designations for the first four orbital quantum numbers with the number of electrons

per orbital at each sublevel are

s:2, p:6, d:10, and f:14

### The maximum number of electrons that can occupy the 5 orbitals at each energy level is

two, if they have opposite spins

###
The spin quantum number indicates that the number of possible orientations for an electron

in an orbital is

2

###
When n represents the principal quantum number of an energy level, the number of electrons

per energy level is

2n^2

###
The quantum number that indicates the position of an orbital about the three axes in space is

the ____quantum number

magnetic

###
The number of different sublevels within each energy level of an atom is equal to the value of

the ____quantum number.

principle

### The statement that an electron occupies the lowest energy orbital that can receive it is

the Aufbau principle

### In the correct electron-dot notation for the phosphorus atom

one pair of dots and three single dots

###
The electron-configuration notation for scandium (atomic number 21) would show the three

highest energy electrons to have the notation

3d^1 4s^2

###
In the correct electron-dot notation for sulfur (atomic number 16), the symbol S is surrounded

by

two pairs of dots and two single dots

###
If the highest main energy level of an atom has the sand p orbitals filled with electrons, it is

said to have an

octet

###
"Orbitals of equal energy are each occupied by one electron before anyone orbital is occupied by a second electron

and all electrons in singly occupied orbitals must have the same spin" is a statement of

hunds rule

### The electron configuration for the carbon atom (C) is 1s^2 2s^2 2p^2. The atomic number of carbon is

6

### The electron-configuration notation for the element with atomic number 11 is

1s^ 2s^2 2p^6 3s^1