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67 Cards in this Set
- Front
- Back
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What is Atomic Number?
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# protons
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What is Mass Number?
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# protons + # neutrons
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For
A Z X What does each symbol represent? |
A: Mass # (protons + neutrons)
X: Element Z: Atomic # (protons) |
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Compare the mass of an electron, proton and neutron to one another.
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Proton and neutron have almost equal mass; Electron is very small (almost 0)
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How many electrons, protons, and neutrons are in nickel-58?
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28 protons
28 electrons 30 neutrons |
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How many electrons, protons, and neutrons are in nickel-60 2+?
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28 protons
26 electrons 32 neutrons |
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How does 1 amu compare to the atomic weight of carbon-12?
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1 amu = 1/12 atomic weight of 1 mol of C-12
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What does Planck's quantom theory state?
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Energy released as EM radiation comes in bundles called QUANTA
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Equantum = ?
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hf, where h is Planck's constant and f is the frequency of radiation
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How does the energy of an electron relate to its radius of orbit?
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Directly: If the radius of orbit is decreased, then it's energy will also decrease.
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What is an atomic emission spectrum?
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Energy released by an electron as it falls from an excited state to its ground state.
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What is an atomic absorption spectrum?
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When an electron becomes excited, it absorbs energy at a specific wavelength, this is known as an absorption spectrum.
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Why is the Borh model inapplicable to atoms other than hydrogen?
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Because the model didn't take electron repulsion into account (i.e., atoms with more than 1 electron)
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What does the modern quantum model state regarding electron path?
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Electrons do not travel in a fixed, circular orbit around a nucleus, rather they are in rapid motion around region orbitals.
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What does the Heisenberg Uncertainty Principle state?
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Impossible to determine the momentum and position of an electron simultaneously as they are constnatly changing.
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What does the Pauli Exclusion Principle state?
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No 2 electrons in a given atom can possess the same 4 quantum numbers.
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What is the maximum number of electrons in an energy level?
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2n^2, where n is the principal quantum number.
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Is there a greater difference in energy between n=3 and n=4 or n=2 and n=3? Why?
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Between n=2 and n=3, because energy between orbitals decreases as the distance from the nucleus increases.
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What are the maximum number of electrons in a subshell?
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4l+2, where l is the Azimuthal QN
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What are all possible values of the magnetic quantum number?
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-l to l
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What does Hund's rule state?
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Within a given subshell, orbitals are filled such that there are a maximum number of 1/2 filled orbitals with parallel spins.
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What does the Periodic Law state?
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the chemical properties of elements depend on their atomic numbers
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What happens to the numbers of valence electrons as you go across a period? What effect does this have on the attraction between valence electrons and the nucleus?
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Increase number of valence electrons; increase attraction (more tightly bound)
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What happens to the number of valence electrons as you go down a group? What effect does this have on the attraction between valence electrons and the nucleus?
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Number of valence electrons remain constant, but there is increased shielding by other filled principal orbitals, so there is less attraction between valence electrons and the nucleus (less tightly bound)
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What is the periodic trend of atomic radius?
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Atomic radius decreases across a period and increases DOWN a group
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What is Ionization Energy? How does Ionization Energy relate to how tightly bound an electron is to its nucleus?
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Amount of energy required to remove a valence electron from a gaseuous atom.
The more tightly bound the electron is, the greater the Ionization Energy. |
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What is the periodic trend of Ionization Energy?
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IE increases across a period, and decreases down a group.
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What is Electron Affinity?
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Electron affinity is the amount of energy released when an electron is added to an atom (ease in which an electron is accepted)
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Why do Group I elements have significantly lower Ionization Energies?
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Because they only need to lose 1 electron to achieve noble gas configuration.
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What is Effective Charge?
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The attractive pull of the nucleus for electrons.
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What is the relationship between Effective Charge and Electron Affinity?
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The greater the Zeff, the greater the Electron Affinity
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Why do Group IIA electrons tend to have lower electron affinities?
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They have filled s orbitals, they don't need any more electrons (they're stable)
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What is the approximate electron affinity of a noble gas?
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~0
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What is the approximae electron affinity of a halogen?
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VERY HIGH b/c brings them to octet
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What is electronegativity?
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Electronegativity is the attraction an atom feels for electrons IN A CHEMICAL BOND
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How does Ionization Energy relate to Electronegativity?
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Lower IE means lower EN
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What are the characteristic properties of metals? Where are they found on the periodic table?
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Shiny, solid at Troom (except Hg), High Tmelt, High Tboil, MALLEABLE, DUCTILE (drawn into wires), GOOD CONDUCTORS (valence e's move freely, low IE, low EN; Left & Middle of PT
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What are the characteristic properites of nonmetals? Where are they found on the periodic table?
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BRITTLE, NO LUSTER, high IE, high EN, POOR CONDUCTORS; right of PT
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What are the metalloids?
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B, Si, Ge, As, Sb, Te
Being Sinful Gets Ass Sex and Teets |
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What kind of cations do Group IA elements form? Group IIA?
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Univalent; Divalent
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What are the characteristic properties of the transition elements?
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Very hard, high Tmelt, High Tboil, MALLEABLE, CONDUCTORS, low IE, variety of positively charged (OXIDATION) states
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What atoms are exempt from the octet rule? How many valence electrons would each be 'satisfied' with?
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H (2)
Li (2) Be (4) B (6) P, S (8+)} Incorporates d orbital |
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What are the characteristic properties of ionic compounds?
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High Tmelt, High Tboil (strong ESTATIC forces), CONDUCTORS in liquid and aq state, form crystal lattices (maximize attractive forces and minimize repulsive forces of same charge ions)
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How does the number of electrons shared in a molecular bond affect the bond length?
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Increase number of bonds shared --> decrease length of bond
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What is bond energy?
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Amount of energy required to separate two bonded atoms
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How is bond energy related to the number of electrons shared in a bond?
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Increase # electrons shared increases bond energy
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What are nonpolar covalent bonds? Provide 4 examples.
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Occurs between atoms of same EN, such as in diatomic molecules (H2, O2, N2, Cl2)
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Correlate number of effective pairs with both electron and molecular geometry.
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2: linear,
3: trigonal planar or bent 4: tetrahedral, trigonal pyramidal 5: trigonal bipyramidal 6: octahedral |
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Provide the bond angles for the following molecular geometries:
Linear Trigonal planar Tetrahedral Trigonal bipyramidal Octahedral |
180
120 109.5 90, 120, 180 90, 180 |
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Describe orbital overlap in sigma and pi bonds.
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Sigma : head to head
Pi: parallel |
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Why are IMF less important in gas phase?
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Molecules are too spread apart to exert significan IMF
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How many torrs are in 1 atmosphere?
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760
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What are the conditions for STP?
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273K, 1atm
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What does Boyle's Law state? If graphed, what would the relationship in the eqn look like?
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P1V1=P2V2
Curve (start high to tangential low) |
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What does Charles' Law state?If graphed, what would the relationship in the eqn look like?
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V1/T1=V2/T2
Linear, start low, end high |
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What does Avogadro's Principle state?
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n1/v1 = n2/v2
ALL GASES HAVE THE SAME NUMBER OF MOLECULES IN THE SAME VOLUME |
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What volume does 1 mol of gas have?
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22.4 L
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Using the Ideal Gas Law, how can the density of a gas be determined?
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PV = nRT
n= m/MM d= m/v thus, m/v = P(MM)/RT |
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Using the Ideal Gas Law, how can molar mass be determined?
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PV=nRT
n=m/MM thus, MM= density * RT/P |
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Under what conditions do real gases deviate from ideality?
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Low temperature, High pressure
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How do real gases deviate from ideality as a function of pressure? How would this affect predicted volume?
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At moderately high pressure, volume is less than IGL predicts because of IMF
At REALLY HIGH PRESSURE, size of particles larger than distance between them, increasing volume |
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How do real gases deviate from ideality as a function of temperature? How would this affect predicted volume?
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At lower temperature, molecules move at a lower velocity, allowing for IMF to exert greater effect, thus, smaller volume
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What does Dalton's Law of Partial Pressures state? Define all variables.
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Pt = Pa + Pb Pc...
where Pa = PtXa where Xa = na/ntotal} mole fraction |
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What are the 5 assumptions of the Kinetic Molecular Theory of Gases?
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1) Vgas molecs is negligible to Vcontainer
2) No IMF/repulsion 3) Gas particles in continuous motion & collision 4) Collisions are elastic 5) KE gas is directly proportional to temperature |
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If it is impossible to determine the speed of an individual gas particle, what equation can be used? What does this equation tell us?
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Root mean square:
(3RT/MM)^1/2 Determines the avg KE per particle and then the speed to which it corresponds MUST USE 1J=1kgm^2/s^2kg AND R=8.312 |
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Define diffusion. Provide an equation that describes rate of diffusion of a gas.
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Diffusion: when gas molecules in isobaric conds diffuse through a mixture (open perfume bottle)
r1/r2 = ((MM2)/(MM1))^1/2 Where 1 and 2 are for the two gases. |
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Define effusion. Provide an equation that describes rate of effusion of a gas.
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Effusion: flow of gas under pressure from one compartment to another via a small opening
r1/r2 = ((MM2)/(MM1))^1/2 Where 1 and 2 are for the two gases. |
