Row 1
Energy levels are described as _________ because the energy absorbed or emitted occurs only in certain.
quantized
Bohr’s model accurately illustrated the emission spectra of a(n) __________ atom.
hydrogen
Orbitals with low energies predict that an electron’s _________ distance from the nucleus is small.
average
The s, p, d, and f sublevels are identified by _________ quantum numbers.
principal
When all the orbitals for an atom are combined, a roughly spherical region is produced around the atom called the __________.
electron cloud
The type of sublevel found in all principal energy levels is the _____.
s sublevel
The modern periodic table is a model representing __________.
principal energy levels and energy sublevels
If an atom gains an electron, the atom will have a ___________ charge.
negative
Which sublevel comes after 3p?
4s
helps explain line spectra
Which orbital makes up most of the transition metals?
Which element is 1s^2 2s^2
Beryllium
states that two electrons in the same orbital must have opposite spins
Pauli exclusion principle
has a spherical shape
s sublevel
holds the greatest amount of electrons
f sublevel
has three orbitals
p sublevel
contains only one orbital
s sublevel
The model that suggested that electrons exist only in a series of distinct energy levels known as orbits at increasing distances from the nucleus is the __________.
Bohr Model
An atom’s lowest energy state is its __________.
ground state
The highest number of energy levels that an atom can have at ground state is __________.
seven
The quantum model divides energy sublevels into __________ parts.
four
The p sublevel can hold a maximum of __________ electrons.
six
The maximum number of electrons that each orbital can hold is __________.
two
Electron dot notation is used to represent the __________ in an atom.
valence electron
A negatively charged ion is called a(n) __________.
anion