ACS Chemistry Final Exam

Layout of an element (mass # & atomic #)

atomic number =

# of protons

mass number =

# of protons + neutrons

the number of protons in a neutral atom will equal the

# of electrons

how to find the correct number of neutrons

mass number - atomic number

Forms of the same elements that differ in amount of neutrons

isotopes

What particle, if lost from the nucleus, would NOT cause a change in the atomic number?

a neutron because it has no charge

When alpha particles were shot at a metal foil target, most passed through without deflections, while others deflected at large angles. What did this suggest to Rutherford?

that the atoms of the metal were mostly empty space, while the nucleus consisted of most of the mass which included highly condensed positive particles (which caused the deflection).

An atom has a valence shell configuration of 1s1. To which group of elements on the periodic table does it belong?

IA
alkali metals

electromagnetic spectrum

The greater the wavelength of a photon..?

the lower its frequency

The greater the frequency of a photon...?

the shorter its wavelength

Light energy formula

What does C in the light energy formula represent?

Give the ground-state electron configuration of an atom in the second period

1s2 2s1

Electrons configuration rule that states electrons do not pair until they have to. (put one electrons in each electron domain then pair up)

Hund's rule

An experimental phenomena associated with atoms having unpaired electrons - which states such substances are attracted to magnetic fields

Paramagnetism

Which drop in energy level results in the greatest emission of energy?

n=2 to n=1

quantum numbers

What do the 4 quantum numbers stand for?

n = energy level
l = (n-1)
ml -l to l
mn 1/2 or -1/2 (spin)

List the quantum numbers for the s, p, d, and f orbitals

s 1,0,0
p 2, 1, -1-0-1
d 3, 2, -2--1-0-1-2
f 4, 3 -3--2--1-0-1-2-3

Py orbital

Which element is represented by X

Chromium

What two subatomic particles have the most mass, but occupy very little of the volume of an atom

protons and neutrons

Define Isoelectronic

Having the same amount of electrons

How does a sodium ion differ from a sodium atom?

the sodium ion has fewer electrons

two or more compounds with the same formula but a different arrangement of atoms in the molecule and different properties

isomer

two or more different physical forms in which an element can exist. Graphite, charcoal, and diamond are all ________ of carbon.

allotropes

What makes up an alpha particle?

2 protons and 2 neutrons

What did Millikan discover from his oil drop experiments?

the magnitude of the charge on an electron

Periods vs Groups

when an atom of an electropositive atom becomes an ion it..?

becomes larger

Nearly all the mass in an atom is located _________ because both ______ & ______ are located there, and each of these particles have a mass larger than the ______

inside the nucleus
protons & neutrons
electron

Classify the following as an element, compound, or mixture. If it is a mixture, decide if it is a homogeneous or heterogeneous mixture.

1 Sugar
2 Spaghetti Sauce
3 Phosphorus

1 compound, not a mixture
2 mixture, heterogenous
3 element

Properties that do depend on the amount of matter present.

extensive

Dz^2 orbital

Dxy orbital

Dx^2y^2 orbital

List the shape, electron domain geometry, and predicted bond angle of a molecule with 6 electron domains

Octahedral
90º

List the electron domain geometry & molecular geometry of a molecule with 4 electron domains (4 bonding 0 nonbonding)

electron domain geometry: tetrahedral
molecular geometry: tetrahedral

List the electron domain geometry & molecular geometry of a molecule with 4 electron domains (3 bonding 1 nonbonding)

electron domain geometry: tetrahedral
molecular geometry: trigonal pyramidal
ex: NH3

List the electron domain geometry & molecular geometry of a molecule with 3 electron domains (2 bonding 1nonbonding)

electron domain geometry: trigonal planar
molecular geometry: bent

List the electron domain geometry & molecular geometry of a molecule with 3 electron domains (3 bonding 0 nonbonding)

electron domain geometry: trigonal planar
molecular geometry: trigonal planar

List the electron domain geometry & molecular geometry of a molecule with 2 electron domains (2 bonding 0 nonbonding)

electron domain geometry: linear
molecular geometry: linear

List the electron domain geometry & molecular geometry of a molecule with 4 electron domains (2 bonding 2 nonbonding)

electron domain geometry: tetrahedral
molecular geometry: bent/nonlinear
ex: H2O

List the electron domain geometry & molecular geometry of a molecule with 5 electron domains (5 bonding 0 nonbonding)

electron domain geometry: trigonal bipyramidal
molecular geometry: trigonal bipyramidal
ex: PCl5

List the electron domain geometry & molecular geometry of a molecule with 6 electron domains (6 bonding 0 nonbonding)

electron domain geometry: octahedral
molecular geometry: octahedral
ex: SF6

List the electron domain geometry & molecular geometry of a molecule with 6 electron domains (5 bonding 1 nonbonding)

electron domain geometry: octahedral
molecular geometry: square pyramidal
ex: BrF5

List the electron domain geometry & molecular geometry of a molecule with 5 electron domains (2 bonding 3 nonbonding)

electron domain geometry: trigonal bipyramidal
molecular geometry: linear
ex: I3-

List the electron domain geometry & molecular geometry of a molecule with 5 electron domains (3 bonding 2 nonbonding)

electron domain geometry: trigonal bipyramidal
molecular geometry: t-shaped
ex: CIF3

List the electron domain geometry & molecular geometry of a molecule with 5 electron domains (4 bonding 1 nonbonding)

electron domain geometry: trigonal bipyramidal
molecular geometry: see saw shape
ex: SF4

List the shape, electron domain geometry, and predicted bond angle of a molecule with 5 electron domains

trigonal bipyramidal, 120º equitorial & 90º axial

List the shape, electron domain geometry, and predicted bond angle of a molecule with 4 electron domains

tetrahedral 109.5º

List the shape, electron domain geometry, and predicted bond angle of a molecule with 2 electron domains

linear 180º

List the shape, electron domain geometry, and predicted bond angle of a molecule with 3 electron domains

trigonal planar 120º

What does a nonbonding electron domain represent?

a lone PAIR of electrons

What does a bonding electron domain represent?

a bond. single or multiple

how many valence electrons does hydrogen have?

2

Identify the bond that would form between an element with a low ionization energy and an element with a high electron affinity

an ionic bond

What does it mean when an element has a low ionization energy?

It means that it can easily lose electrons

What does it mean when an element has a high electron affinity

It means that it can easily accept electrons to form negative ions

The type of bond that results when both elements contribute electrons to form a shared pair

covalent bonds

The type of bond that results when both elements contribute electrons but one element furnishes both electrons

coordinate covalent bond

High energy photons have enough energy to do what?

disrupt covalent bonds

What has to be true of a non polar molecule that has polar bonds

it must be symmetric enough so that all the dipoles cancel out

a molecule in which a concentration of positive electric charge is separated from a concentration of negative charge.

dipole

What type of compound is expected to have the largest dipole movement?

a bent compound

The boiling point of H2O, compared with other members of the series can be explained by

hydrogen bonding

How do you calculate formal charge?

(#of valence electrons) - (nonbonding electrons) - (bonding electrons / 2)

a triple bond is made up of

2 pi bonds
1 sigma bond

a double bond is made up of

1 sigma
1 pie

What is the molar volume of a gas?

22.4 L

If a 17.0g of impure Ni+ metal reacts with excess carbon monoxide, CO, forming 6.25 L of Ni(CO)4 gas under standard temperature and pressure conditions, what is the percent by mass of Ni+ in impure nickel metal sample?

What do you start the stoich equation?

6.25 L Ni(CO)4

What is the main gas law equation?

PV=nRT

(pressure x volume) =

What is the equation for Pressure?

Force/Area

Gas Law: Temperature-Volume relationship, at constant pressure. What is the constant for Charle's Law?

V/T = constant

Gas Law: Pressure-Volume relationship, at constant temperature. Boyle's Law

PV = constant

Gas Law: Pressure- Temperature relationship, at constant volume. Gay-Lusaacs' Law

P/T = constant

Temperature in Gas Law equations must be in what type of measurement? What is the conversion?

Must be in Kelvin
273.15 + C = K

P1V1 will always equal________ if temperature and particle numbers are constant

P2V2

1 atm = ? kPA?

101.325

What does R equal when dealing with meters/mol K
(m^3/mol)

8.3145

What does R equal when dealing with Liters kPA/mol K
(L/mol K)

8.3145

What does R equal when dealing with Liters atm/ mol K

.082

Solubility: NO3-

Nitrate is soluble

Solubility: C2H3O2

Methyl carbonate is soluble

Solubility of Cl- Br- I-

Soluble except in Ag2+, Pb2+, Hg2+

Solubility of SO4 2-

Sulfate is soluble except in Sr2+, Hg2+, Ba2+, Pb2+, Ca2+

Solubility of OH- and O2-

Hydroxide and Peroxide are insoluble except with alkali metals, Ca2+, Sr2+, Ba2+

Solubility of PO4 3-

Phosphate is insoluble EXCEPT with NH4+ and alkali metals
(Ammonium, and Group 1 metals)

Solubility of CO 3-

Carbonate is insoluble EXCEPT with NH4+ and alkali metals
(Ammonium, and Group 1 metals)

Solubility of SO3 2-

Sulfite is insoluble EXCEPT with NH4+ and alkali metals
(Ammonium, and Group 1 metals)

Solubility of S 2-

Sulfur is insoluble EXCEPT with NH4+, alkali metals,
(Ammonium, Group 1)

2 electron domains results in what type of hybridization?

sp

6 electron domains results in what type of hybridization?

Sp3d2

reaction in which electrons are transferred from one reactant to the other

redox reactions

Assigning Oxidation Numbers Rules (3)

1. all elements in elemental form have an oxidation # of zero
2. For a monotonic ion the oxidation number equals the charge on the ion
3. The sum of the oxidation numbers in a molecule will equal the charge on the molecule

Assigning Oxidation Number Rule Exceptions

Oxygen = -2 except in Peroxide = -1
Hydrogen = +1 when with nonmetal -1 when with metal
Halogens are -1 except when with Oxygen while Fluorine is ALWAYS -2

What does the Reducing Agent do in a redox reaction? (aka the Reductant)

gives away an electron. Becomes oxidized

What does the Oxidizing Agent do in a redox reaction?
(aka the oxidant)

gains an electron. Becomes reduced