Section 1
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Give the ground-state electron configuration of an atom in the second period
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Cards (182)
Section 1
(50 cards)
Give the ground-state electron configuration of an atom in the second period
1s2 2s1
Dz^2 orbital
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
electromagnetic spectrum
atomic number =
# of protons
List the shape, electron domain geometry, and predicted bond angle of a molecule with 6 electron domains
Octahedral 90º
Properties that do depend on the amount of matter present.
extensive
Forms of the same elements that differ in amount of neutrons
isotopes
quantum numbers
when an atom of an electropositive atom becomes an ion it..?
becomes larger
mass number =
# of protons + neutrons
What makes up an alpha particle?
2 protons and 2 neutrons
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).
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
Which element is represented by X
Chromium
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
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)
Dx^2y^2 orbital
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
how to find the correct number of neutrons
mass number - atomic number
Periods vs Groups
An atom has a valence shell configuration of 1s1. To which group of elements on the periodic table does it belong?
IA alkali metals
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
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
Light energy formula
What does C in the light energy formula represent?
the number of protons in a neutral atom will equal the
# of electrons
What did Millikan discover from his oil drop experiments?
the magnitude of the charge on an electron
An experimental phenomena associated with atoms having unpaired electrons - which states such substances are attracted to magnetic fields
Paramagnetism
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 (4 bonding 0 nonbonding)
electron domain geometry: tetrahedral molecular geometry: tetrahedral
Which drop in energy level results in the greatest emission of energy?
n=2 to n=1
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 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 5 electron domains (5 bonding 0 nonbonding)
electron domain geometry: trigonal bipyramidal molecular geometry: trigonal bipyramidal ex: PCl5
Layout of an element (mass # & atomic #)
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
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-
The greater the wavelength of a photon..?
the lower its frequency
Py orbital
Dxy orbital
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
What particle, if lost from the nucleus, would NOT cause a change in the atomic number?
a neutron because it has no charge
The greater the frequency of a photon...?
the shorter its wavelength
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
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
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
two or more different physical forms in which an element can exist. Graphite, charcoal, and diamond are all ________ of carbon.
allotropes
Section 2
(50 cards)
What is the molar volume of a gas?
22.4 L
List the shape, electron domain geometry, and predicted bond angle of a molecule with 3 electron domains
trigonal planar 120º
Gas Law: Pressure-Volume relationship, at constant temperature. Boyle's Law
PV = constant
The type of bond that results when both elements contribute electrons to form a shared pair
covalent bonds
a double bond is made up of
1 sigma 1 pie
Solubility of OH- and O2-
Hydroxide and Peroxide are insoluble except with alkali metals, Ca2+, Sr2+, Ba2+
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 R equal when dealing with Liters atm/ mol K
.082
how many valence electrons does hydrogen have?
2
How do you calculate formal charge?
(#of valence electrons) - (nonbonding electrons) - (bonding electrons / 2)
What does it mean when an element has a low ionization energy?
It means that it can easily lose electrons
What does a bonding electron domain represent?
a bond. single or multiple
P1V1 will always equal________ if temperature and particle numbers are constant
P2V2
a molecule in which a concentration of positive electric charge is separated from a concentration of negative charge.
dipole
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
Solubility of SO3 2-
Sulfite is insoluble EXCEPT with NH4+ and alkali metals (Ammonium, and Group 1 metals)
The type of bond that results when both elements contribute electrons but one element furnishes both electrons
coordinate covalent bond
What does R equal when dealing with Liters kPA/mol K (L/mol K)
8.3145
When rounding to 3 sig figs, if you have a number that is .9647
What does a nonbonding electron domain represent?
a lone PAIR of electrons
List the shape, electron domain geometry, and predicted bond angle of a molecule with 5 electron domains
trigonal bipyramidal, 120º equitorial & 90º axial
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
Solubility of S 2-
Sulfur is insoluble EXCEPT with NH4+, alkali metals, (Ammonium, Group 1)
What is the main gas law equation?
PV=nRT (pressure x volume) =
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)
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
2 electron domains results in what type of hybridization?
sp
List the shape, electron domain geometry, and predicted bond angle of a molecule with 2 electron domains
linear 180º
Solubility of SO4 2-
Sulfate is soluble except in Sr2+, Hg2+, Ba2+, Pb2+, Ca2+
Gas Law: Temperature-Volume relationship, at constant pressure. What is the constant for Charle's Law?
V/T = constant
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
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
Temperature in Gas Law equations must be in what type of measurement? What is the conversion?
Must be in Kelvin 273.15 + C = K
The boiling point of H2O, compared with other members of the series can be explained by
hydrogen bonding
What is the equation for Pressure?
Force/Area
1 atm = ? kPA?
101.325
reaction in which electrons are transferred from one reactant to the other
redox reactions
What does R equal when dealing with meters/mol K (m^3/mol)
8.3145
Solubility: NO3-
Nitrate is soluble
List the shape, electron domain geometry, and predicted bond angle of a molecule with 4 electron domains
tetrahedral 109.5º
What does it mean when an element has a high electron affinity
It means that it can easily accept electrons to form negative ions
Solubility: C2H3O2
Methyl carbonate is soluble
Solubility of Cl- Br- I-
Soluble except in Ag2+, Pb2+, Hg2+
6 electron domains results in what type of hybridization?
Sp3d2
Gas Law: Pressure- Temperature relationship, at constant volume. Gay-Lusaacs' Law
P/T = constant
What type of compound is expected to have the largest dipole movement?
a bent compound
High energy photons have enough energy to do what?
disrupt covalent bonds
a triple bond is made up of
2 pi bonds 1 sigma bond
Section 3
(50 cards)
What type of bond has a low conductivity as a solid but a high conductivity when fused?
ionic Ex: NaCl
The _____ is titrated with the ______
titrand titrant
Define electropositive atoms. Where are they located
smallest value, least electronegative. Located bottom left of periodic table
Which type of compound has a higher melting point?
ionic compounds have higher melting points that molecular compounds
measure force of gravity of an object
weight
How did Thompson discover the Electron?
by cathode
contains more dissolved solute than a saturated solution at that temperature.
supersaturated solution
A solution will conduct electricity if it contains what?
dissolved ions
What are rows What are columns
periods are rows groups of columns
How do you calculate Molarity
mol/L
Can be observed without changing the identity & composition of a substance
Physical property (color, density, melting point) all intensive. do not depend on amount of substance e
equal volumes of gas under the same temperature and pressure will have...?
the same amount of molecules (avagondros)
What does a neutralization reaction occur between? What does it result in?
strong acid + base H2O
List the 7 strong acids
HCl - hydrochloric acid HBr - hydrogen bromide HI - hydrogen iodide HClO3 - Chloric acid HClO4 - Perchloric acid HNO3 - Nitric acid H2SO4 - Sulfuric acid
The ______ is dissolved in the _______
solute solvent
Bond formed from: metal+nonmetals
ionic bond
The strong bases are what?
soluble group 1 group 2 metal hydroxides
poor conductors, brittle
nonmetal
Energy is required to
break a bond
the energy released when one mole of an ionic solid is formed from gaseous ions. Measures the strength of an ionic bond
Lattice energy
Describe the atom. What makes up the nucleus and where do electrons reside
Protons and neutrons form the small, dense nucleus; electrons are found in a diffuse cloud around the nucleus; most of the volume of an atom is empty space.
measure of how much matter an object contains
mass
What do neutralization reactions take place in
acid + base leaving salt + water
an analytical technique to determine the concentration of a solute.
Titration
What is the equation for dilution
(moles solute before dilution) = (moles solute after dilution) C1V1 = C2V2
formula for q
specific heat formula
δ+ goes over the ____________ and δ- over the ___________ atom
electropositive, electronegative
Has two ionizable protons (H2SO4)
Diprotic acid
contains less dissolved solute than a saturated solution at that temperature
unsaturated solution
Acids increase the concentration of what? Bases increase the concentration of what?
H+ OH-
Thompson discovered the Plum Pudding Model - what was that? Who proved him wrong?
stated that nucleus was a scattered positive sphere with electrons embedded in it, was proved wrong by Rutherford who did the gold foil experiment
What effects the vapor pressure of a liquid
temperature
What is the molecular weight?
the sum of the mass of each element
Who discovered the proton?
Rutherford by bombarding N2 with alpha particles
An ionic bond is stronger (i.e. the lattice energy is more negative) if:
1) The charge on the individual ions is greater 2) The distance between + and - charge is less (smaller ions)
Who discovered the nucleus by observing the scattering of α-particles off of a thin gold foil & discovered the proton by bombarding N2 with α-particles.
Rutherford
What is one weak base you should memorize
NH3 (ammonia)
What does the Oxidizing Agent do in a redox reaction? (aka the oxidant)
gains an electron. Becomes reduced
Energy is released when
a bond forms
Define Bond Polarity
Electrons will spend most of their time around the most electronegative atom
Cannot be observed without changing the identity & composition of a substance
chemical property
What does a low vapor pressure value indicate (little tendency to change from liquid to gas)
higher heat of vaporization higher boiling points high surface tension
bond formed from: two nonmetals
molecular compound
a substance that produces ions when dissolved in solution.
an electrolyte
α-particles β-particles γ-rays
2+ elementary charge 1- elementary charge uncharged
What does a high vapor pressure value indicate
lower heats of vaporization lower boiling points less surface tension
Why are lattice energies listed as positive values instead of negative values?
This represents the energy needed to break apart one mole of substance, rather than the energy released when the substance forms.
Electronegativity periodic trend
electronegativity is greater the higher up on the right of the periodic table
an electronegativity difference ≥ 1.7 indicates an ________ (sometimes you see 2.0 instead of 1.7). An electronegativity difference ≤ 0.5 is generally considered ___________. If it is somewhere in the middle it is considered ________
ionic nonpolar polar
Section 4
(32 cards)