Chapters 4-9 Flashcards
What particles are found in the nucleus of an atom?
Protons and neutrons
The atomic number of an element is the total number of which particles in the nucleus?
Protons
What does the number 84 in the name krypton-84 represent?
The mass number
What is the mass number made of?
Protons+neutrons
How does the energy of an electron change when the electron moves closer to the nucleus?
It decreases
The principal quantum number indicates what property of an electron?
Energy level
How many energy sub levels are in the second principle energy level?
2
What is the maximum number of F orbitals in any single energy level in an atom?
7
What is the maximum number of D orbitals in a principal energy level?
5
What is the maximum number of orbitals in the P sub level?
3
What is the maximum number of electrons in the second principal energy level?
8
When an electron moves from a lower to a higher energy level, the electron
Absorbs a quantum of energy
The shape of an electron cloud is determined by the electron’s
Energy sub level
The letter p in the symbol 4p^3 indicates the
Orbital shape
What types of atomic orbitals are in the third principal energy level?
S, P, and D only
Aufbau principal
Electrons enter orbitals of lowest energy first
How does the speed of visible light compare with the speed of gamma rays?
Speed of gamma ray’s is greater
Which color of visible light has the shortest wavelength?
Violet
Which electromagnetic wave has the highest frequency?
Gamma rays
Emission of light from an atom occurs when an electron
Drops from a higher to a lower energy level
As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit
Increase
Which variable is directly proportional to frequency?
Energy
Bohr’s model could only explain spectra of which type of atoms?
Single atoms with one electron
Each period(row) in the periodic table corresponds to a
Principal energy level
How does atomic radius change from top to bottom in a group(column) in the periodic table?
It tends to increase
Electrons
Mass: 0amu
Charge: -1
Protons
Mass: 1amu
Charge: +1
Neutrons
Mass: 1amu
Charge: 0
What is the atomic mass?
Weighted average of all isotopes
4 quantum numbers
n
L
mL
mS
N
Principle quantum number
Energy level
Any integer above 0
L
Shape
Subshell
0
L=0
S
L=1
P
L=2
D
L=3
F
mL
Orbital
Can hold 2 electrons
-L
mS
Spin
No 2 identification electrons
mS=-1/2, +1/2
Frequency
ν
Cycles/seconds
Wavelength
λ
Unit of energy
Joules
Energy
E=hν
Frequency
ν=c/λ
Cation
+
Anion
-
Atomic size/radius
Increases downward and from right to left
Ionization energy
Energy required to steal an electron from that atom
Increases from bottom to top, left to right
Electronegativity
How much it wants to steal an electron
Increases from top to bottom, left to right
Ionic compounds are usually in what state?
Gas
What particles are free to drift in particles?
Electrons
What characteristic of metals make them good electrical conductors?
They have mobile valence electrons
What information does a molecular formula provide?
Number and kind of atoms present in a molecule
What is shown by the structural formula of a molecule?
The arrangement of bonded atoms
The chemical formula of an ionic compound shows
The lowest whole-number ratio between ions in the ionic compound
What is thought to cause dispersion forces?
Motion of electrons
Which of the forces of molecular attraction is the weakest?
Dispersion
What type of ions have name sending in -ide?
Only anions
Sulfur hexafluoride is an example of a
Binary compound
Binary molecular compounds are made of two
Nonmetallic elements
Diatomic elements
Hon halogens
Steric number
Number of things it’s bonded to + lone pairs
Covalent bonds
Have prefixes
Ate
ic acid
ite
ous acid
ide
hydro- -ic acid
