Gen Chem 2- Test 2 – Flashcards

Unlock all answers in this set

Unlock answers
question
Electron configuration
answer
Distribution of electrons in an atom/molecule in their orbitals
question
Ground state
answer
Electron configuration with the lowest energy levels
question
Orbital diagram
answer
A diagram of the electron population within the orbitals
question
Electron spin
answer
m sub s, an upwards or downwards arrow
question
Pauli exclusion principle
answer
no two electrons can have the same quantum numbers
question
Periodic law
answer
Elements with sumilar physical/chemical properties fall within the same column (up and down on per. table)
question
Aufbau principle
answer
Fill the lowest energy levels first
question
Valence electrons
answer
Electrons in the outermost shell
question
Hund's rule
answer
Electrons are placed individually in orbital diagrams until full
question
Noble gas orbital diagrams are
answer
Stable (full)
question
n
answer
energy level
question
l
answer
orbital type
question
m sub l
answer
orientation
question
m sub s
answer
electron spin
question
Dmitri Mendeleev
answer
Created the modern periodic table
question
What did the periodic law do?
answer
It allowed for predictions not yet discovered
question
order of energy levels
answer
s, p, d, f
question
core electrons
answer
electrons that are not valence electrons
question
How do valence electrons explain periodic law?
answer
Elements in the same column/family have same v.e. #, similar properties
question
Anomalous electron config.
answer
S-orbital partially fills before d-orbital begins to fill, or s-orbital is skipped
question
How do valence electrons explain periodic law?
answer
Elements in the same column/family have same v.e. #, similar properties
question
Anomalous electron config
answer
S-orbitals only partially filled before electrons move to d-orbital, or s-orbital skipped
question
5 anomalous elements
answer
Chromium, copper, silver, gold, and paladium.
question
Config of the 5 anomalous elements
answer
Cr= [Ar] 4s1 3d5
Cu= [Ar] 4s1 3d10
Ag= [Kr] 5s1 4d10
Au= [Xe] 6s1 5d10
Pd= [Kr] 4d10
question
Cation
answer
Element with a positive charge due to losing an electron
question
Anion
answer
Element with a negative charge due to gaining an electron
question
Octet
answer
8 valence electrons
question
Duet
answer
2 valence electrons (helium)
question
What tends to form cations?
answer
Metals
question
What tends to form anions?
answer
Nonmetals
question
Group 1A and 2A lose what valence electrons to form cations?
answer
S-orbital
question
D-block (transition metals) lose what electrons first, and then the next?
answer
S, then D
question
Paramagnetism
answer
Attracted to magnetic field because of unpaired electrons
question
Dimagnetism
answer
Repelled by magnetic field due to all paired electrons
question
Effective nuclear charge
answer
Pull/force an electron "feels" from the nucleus due to protons
question
The pull on electrons is greater when
answer
closer to the nucleus, or less core electrons
question
the pull on electrons is weaker when
answer
farther from nucleus, or more core electrons
question
which electrons feel more Zeff?
answer
core
question
which electrons feel less Zeff?
answer
valence
question
Shielding/screening
answer
Outer valence e- don't feel the charge of the nucleus due to core e-
question
Atomic radius
answer
Gives indication of size of atom
question
The atomic radius is larger when what is weaker?
answer
Zeff
question
The atomic radius is smaller when
answer
The Zeff is greater
question
What causes the atomic radius to be larger or smaller?
answer
The number of electrons inbetween the valence and nucleus
question
Which ion is smaller and why
answer
Cations- they lose electrons
question
Which ion is larger and why
answer
Anions- they gain electrons
question
Which is larger- Br- or Kr?
answer
Bromine, both have the same amount of electrons but Krypton has more protons, so Bromine is larger
question
Which is larger- Li or Ne?
answer
Ne
question
Ionization energy
answer
Energy required to remove an electron from an atom
question
As Zeff increases, what gets stronger?
answer
Ionization energy
question
Why does IE become stronger when Zeff increases?
answer
When an electron is pulled away, the Zeff force gets stronger due to protons, so the energy required to pull away an electron is greater.
question
In terms of heat, IE is
answer
endothermic
question
Why is IE endothermic?
answer
IE means it's doing work on the system in order to remove the electron
question
Electron affinity
answer
Change in energy when an atom gains an electron to form an anion
question
In terms of heat, electron affinity is
answer
either exothermic or endothermic
question
When it comes to electron affinity, what family tends to be exothermic?
answer
noble gases
question
EA becomes more _____ across a period
answer
negative
question
Negative energy in terms of EA tells us what?
answer
It's an exothermic reaction
question
Periodic trend
answer
Trend occurring from left to right- rows
question
Periodic trend for atomic radius
answer
As the # of electrons goes up, the radius becomes larger.
question
Periodic trend for ionization energy
answer
As you go from left to right, ionization energy takes less force because there are more electrons and less force from Zeff
question
Why do atoms bond?
answer
Achieve octet
question
Achieving an octet maximizes ______ and minimizes ______
answer
Attraction, repulsion
question
Ionic bond
answer
Bond between a metal and nonmetal where the electron(s) are transferred.
question
Covalent bond
answer
Bond between two nonmetals- shared.
question
Metallic bond
answer
Bond among metals, communal sharing
question
Most molecular bonds are
answer
Polar
question
Polar bonds are inbetween what?
answer
Covalent and ionic
question
Important physical property of ionic compounds
answer
Conducive of electricity in aqueous conditions
question
Covalent bonding is a result of what?
answer
Overlap of atomic orbitals
question
Physical property of covalent compounds
answer
Poor conductors
question
Examples of metallic bonders
answer
Iron, copper, silver, gold
question
Physical properties of metallic bonders
answer
Malleable, ductile, can conduct heat and electricity
question
Electronegativity
answer
Ability of an atom in a bond to attract electrons to itself
question
Dipole moment
answer
Separation of charges
question
When does a dipole occur?
answer
One side of a molecule is +, and the other side is -
question
Electronegativity increases across a _____ and up a _____
answer
Period, column
question
0-.4
answer
Nonpolar
question
.5-1.9
answer
Polar
question
> or equal to 2.0 (electronegativity)
answer
ionic
question
Why do chemical bonds form?
answer
They lower the potential energy between the charged particles.
Get an explanation on any task
Get unstuck with the help of our AI assistant in seconds
New