Term
When two like charges interact, which combo gives it the highest energy?
small/large charge & close/far |
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Definition
Large charges close together |
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Term
| When two particles move through a magnetic field, and one particle is refracted twice as far as the other, what two differences between the particles is possible? |
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Definition
| One may be twice the charge or twice the mass (this one will refract twice as much). |
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Term
| Which subatomic particles are responsible for the mass of an atom? |
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Definition
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Term
What transition combo is the absorption process that requires the most energy?
From a higher/lower n to a higher/lower n in a higher/lower level of n. |
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Definition
From a lower n value to a higher n in a lower level of n.
Ex: n=1 → n=3 |
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Term
| How would you describe the location cloumn of K on the periodic table? |
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Definition
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Term
| If element A has valence electrons at a higher level then B, then which has the higher ionization energy? |
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Definition
| Because A has a higher valence electon level, it has the higher ionization energy. |
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Term
| Which corner of the periodic table has the highest electronegativity? |
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Definition
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Term
| How would you find elements whose highest occupied orbital is the 4p orbital when in ground state? |
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Definition
| Find the p-block (rightmost block) and count down four rows. All the elements in this row and block have the highest occupied orbital of 4p. |
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Term
| How do you know an ionic compound from another compound? |
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Definition
| An ionic compound will be made of a metal and non-metal. |
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Term
| What orbital letters can hold how many pairs of electrons? |
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Definition
s: 1 pairs
p: 3 pairs
d: 5 pairs |
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Term
| How do you figure out what the greatest mass is amongst elements given in moles, number of atoms, and mass? |
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Definition
Convert the number of atoms into moles (divide by 6.02×1023)
Convert the moles into grams (multiply by the elements' molar masses) |
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Term
| How do you compare the number of atoms in samples of atoms in grams, moles, and number of atoms. |
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Definition
You can easily convert them to moles.
To convert grams to moles, divide by the elements' molar masses.
To convert number of atoms to moles divide by 6.02×1023. |
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Term
| What corner of the periodic table has atoms with the largest radius and what charge increases atomic radii? |
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Definition
| Bottom-left corner. A negative charge increses the size of the radius. |
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Term
| How can you tell if a bond has more ionic character or covalent character? |
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Definition
| The greater the difference in electronegativity between the two atoms, the more ionic the character. The closer the electronegativities, the more covalent the character. |
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Term
| The n=1 level is higher for atoms in what corner of the periodic table? |
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Definition
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Term
| When n=1 is high and a transition is made from n=2 → n=1, will the photon from that trasition be at high or low energy? |
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Definition
| It will be at low energy. |
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Term
| How do you find the number of valence electrons in a element's atom? |
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Definition
| Count on that elements row from left to right. The number of elements you counted is the number of valence electrons. |
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Term
| To find the number of atoms in a compound, what to you do? |
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Definition
| Take the number of "ingredients" (like 2 hydrogen and 1 oxygen for H2O) and multiply it by the number of moles. Then you can convert moles to number of atoms (6.02×1023) |
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Term
| If a atom is in a bond and has two attachments (either single, double, or triple bonds or lone pairs) what is it's bond angle? |
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Definition
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Term
| If an atom is bonded and has three parts (either single, double, or triple bonds or lone pairs), what is the bond angle? |
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Definition
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Term
| If an atom is bonded and has four parts (either single, double, or triple bonds or lone pairs), what is the bond angle? |
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Definition
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Term
| If an atom is bonded and has two parts (either single, double, or triple bonds or lone pairs), what is the hybridization? |
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Definition
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Term
| If an atom is bonded and has three parts (either single, double, or triple bonds or lone pairs), what is the hybridization? |
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Definition
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Term
| If an atom is bonded and has four parts (either single, double, or triple bonds or lone pairs), what is the hybridization? |
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Definition
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Term
| What are the number of sigma and pi bonds in single, double, and triple bonds? |
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Definition
single: 1σ
double: 1σ 1π
triple: 1σ 2π |
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Term
| How can a bond order can be found? |
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Definition
| Take the average of all possible bonds. |
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Term
| In sigma bonding, where is the electron density concentrated? |
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Definition
| The most density is concentrated between the two nuclei. |
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Term
| In pi bonding, where is the electron density concentrated? |
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Definition
| It is concentrated above/below the two nuclei. |
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Term
| Antibonding diagrams are shown how? |
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Definition
| With two similarly colored orbitals overlapping each other. |
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Term
| How does hydrogen bonding arise? |
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Definition
| Hydrogen bonding forces arise from the interaction of a hydrogen atom with a lone pair on a neighboring molecule. |
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Term
| Molecules with the highest boiling point have what kind of bonding? |
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Definition
1: Hydrogen bonding
2: Dipolar bonding
3: Dispersion forces
(weight is also a factor) |
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Term
| The simple cubic cell has what coodination number and packing efficiency compared to the other cubic cells? |
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Definition
| Simple cubic has the smallest coordination number and the worst packing efficiency. |
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Term
| The body centered cubic cell has what coodination number and packing efficiency compared to the other cubic cells? |
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Definition
| Body centered cubic cells have the middle coordination number and the medium packing efficiency. |
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Term
| The face centered cubic cell has what coodination number and packing efficiency compared to the other cubic cells? |
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Definition
| The face centered cubic cell has the largest coordination number and the greatest packing efficiency. |
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Term
| What is the simple cubic cell's coordination number? |
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Definition
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Term
| What is the body centered cell's coordination number? |
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Definition
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Term
| What is the face centered cubic cell's coordination number? |
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Definition
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Term
| The less conductive a material, the larger or smaller the bandgap? |
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Definition
| The bandgap is larger in materials that do not conduct well. |
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Term
| Molecular solids tend to have what kind of boiling points? |
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Definition
| Molecular solids have relatively low, normal boiling points. |
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Term
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Definition
| It is the change in enthalpy. Enthalpy is the sum of kinetic and potential energy. |
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Term
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Definition
| It is the change in entropy. Entropy is the number of ways molecules can be arranged in a system. |
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Term
| If a weak bond is broken and a strong bond is formed, what is the most likely tempurature exchange? |
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Definition
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Term
| If a strong bond is broken and a weak one forms, what is most likely tempurature exchange? |
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Definition
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Term
| What is the equation for finding ΔH from bond energies? |
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Definition
ΔH
≈
∑(broken bond energies)
-
∑(formed bond energies) |
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Term
| If ΔH is positive, what was the heat transfer? |
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Definition
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Term
| If ΔH is negative, what was the heat transfer? |
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Definition
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Term
What is the equation for the Second Law of Thermodynamics concerning free energy?
(Used to calculate spontaneity) |
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Definition
ΔG = ΔH - T×ΔS
If ΔG is negative, the reaction is spontaneous (and vice-versa). |
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Term
| What is the difference between ΔG and ΔG°? |
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Definition
| ΔG° is for specific amounts of reactant and product, ΔG is for unspecified amounts. |
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Term
| If a reversible reaction's ΔG° is negative, then what is K in relation to 1 at equilibrium? |
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Definition
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Term
| If a reversible reaction's K value is greater than 1, then what is true about the activation energy at equilibrium? |
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Definition
| The activation energy of the foreward reaction is less than that of the reverse reaction. |
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Term
| When you increase tempurature, what happens to the number of collisions in a system? |
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Definition
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Term
| How does a catalyst help a reaction? |
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Definition
| It orients molecules porperly to speed up a reaction. |
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Term
| If you decrease the concentration of reactants, what will happen to the speed of the reaction? |
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Definition
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Term
| If a reaction has a high activation energy, then what can you conclude about the reaction rate? |
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Definition
| It has a very low reaction rate. |
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Term
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Definition
| They form a micelle with hydrocarbon tails pointing inwards. |
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Term
| What is Avagadro's Number? |
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Definition
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Term
| What is Coulomb's Law concerning force? |
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Definition
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Term
| What is Coulomb's Law concerning energy? |
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Definition
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