Bonding, IMF, VSEPR, Organic Chem, Solutions, Gases
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| What does a "polar molecule" mean? | A polar molecule is a molecule which has two opposite sides that are non symmetrical. One pole is like the "bully", it exerts a more attractive force to the other's electrons, like in water.
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| How can a molecule have no dipole moment | A molecule will have no dipole moment if it's geometry is completely symmetrical, like in linear, tetrahedral, octahedral or t-shapes.
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| What are resonance structures? | Different, but valid, Lewis Dot Structures that obey the octet for the same molecule.
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| Why are resonance structures needed? | Electrons are in constant motion, they are never localized, so more than one Lewis Dot diagram is possible.
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| What is the rule for the formal charge? | (Valence e- of the atom) - (valence e- assigned to the atom in the structure)
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| How do you determine which resonance structure is the best? | The formal charges should be as close to zero as possible.
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| What does VSEPR mean (what does it imply about electron placement)? | Non bonded pairs should be as far apart as possible, and each pair should be removed or added as opposites.
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| What does degenerate mean? | It means that [they] are equal.
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| What is hybridization? | When electrons from different orbitals hybridize to form a conjoined orbital, like "s" and "p" combine as "sp" when bonding.
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| Can atoms like O,C,N, or F ever have a dsp3 hybridization? | No, because they do not have a "d" block to which the electrons can move to. The non-metallic elements in period 3, however, do have an empty "d" block, so they can have a dsp3 hybridization.
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| What are sigma bonds? | Single bonds between electrons
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| What are pi bonds? | When double or triple bonds exist, a pi bond is created because the bonds don't actually touch each other. Rather, they are parallel.
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| How many sigma and pi bonds are in a single bond? How many sigma and pi bonds are in a double bond? How many sigma and pi bonds are in a triple bond? | a) 1 sigma bond and 0 pi bonds
b) 1 sigma bond and 1 pi bond
c) 1 sigma bond and 2 pi bonds
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| What are metalloids? | Metalloids are elements which have properties of both metals and non metals, they are: shiny, poor conductivity, malleability
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| How do you know if an element is a metalloid by looking at the Periodic Table? | One side of the element will be touching the staircase.
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| What is the octet rule? | Electrons will lose or gain (cation or anion) electrons to form a stable noble gas with 8 electrons in the valence shell.
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| Describe ionic bonds | -The transfer of electrons
-Metals and nonmetals
-High melting point and boiling point
-Conduct as liquid, mostly solid
-Soluble
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| Describe metallic bonds | -Sea of electrons
-Metals only
-High melting point and boiling point
-Insoluble
-Always conduct, and have other metallic properties
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| Describe covalent bonds | -Share electrons
-Non metals only
-Low melting point and boiling point
-Insoluble unless polar
-Never conduct
-Create molecules
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| If the lattice energy is not enough, can a compound be made? | No, reactions must be exothermic!
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| Which compounds have more lattice energy? | Compounds in which the elements have higher chargers and the distance between atoms are much smaller.
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| What is sublimation? | When a metal goes from the solid phase to the gaseous phase.
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| Are bonds stronger or intermolecular forces? | Bonds are stronger!
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| What do intermolecular forces do? | They hold a substance together, it's the attraction between molecules.
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| Sbstances with strong IMF have (a) melting points, (b) boiling points and are most likely to be (c) at room temperature. | (a) high
(b) high
(c) solids
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| What is London Dispersion? | It is the weakest attraction between covalent (mostly non polar) molecules. The electrons of one atom attract the nucleus of another. This causes a temporary shift of electrons making one side of the molecule positive and the other negative.
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| What makes the London Dispersion force stronger? | If there are more electrons, the force will be stronger.
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| What is a dipole-dipole attraction? | They occur between polar molecules, and are stronger than LDF. The more polar a molecule is, the greater the force of attraction.
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| London Dispersion and Dipole-Dipole can also be called: | Van der Waals forces!
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| What is a hydrogen bond? | A very strong IMF that exists between hydrogen, fluorine, oxygen and nitrogen because the latter three have high electronegativities and make very polar substances. They have high melting and boiling points.
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| In C and SiO2, what happens with the IMF? | Network solids are formed, although they are covalently bonded. The VDW forces are much stronger than normal.
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| What are Ion-Dipole Attractions? | The strongest attraction exists between ionic compounds and polar compounds. Polar substances can ionize ionic substances due to strong attractions.
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| When should you use the Combined Gas Law? | When you are given two different conditions and asked to find a new volume/pressure/temperature.
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| What type of gases travel faster? Which are slower? | Lighter gases are faster. Heavier gases are slower.
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| When should PV=nRT be used? | When you are given information to find only one of the variables. No new and previous conditions.
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| Is PV=nRT reliable although it applies to ideal gases? | Yes, because the values are extremely close!
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| When temperature increases.... | volume increases
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| What are the three characteristics of an ideal gas? | 1. Do not attract or repel.
2. Have negligible volumes
3. Molecules are in constant, rapid, random and straight-line motion
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| When temperature increases.... | pressure increases
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| When pressure increases.... | volume decreases
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| What does Avogadro say about equal volumes of gases at the same temperature and pressure? | They have the same number of molecules
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| What is surface tension? | An elastic force on the liquid surface. The stronger the IMFs, the higher the forces and surface tensions.
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| What is viscosity? | Viscosity is a measure of a liquid's resistance to flow. The greater the IMF, the greater the viscosity and the slower it will flow. If you increase the temperature, viscosity decreases.
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| Define exothermic | When heat is given off (radiated) during a reaction
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| Define endothermic | When no heat is radiated, but a lot was absorbed for the reaction
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| On a phase change diagram, what do straight lines represent? | A phase change
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| How does the cooling curve differ from a heat diagram | They are opposites
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| In a triple point diagram, the triple point is when | a substance can exist as all three states simultaneously
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| In a triple point diagram, the critical point is when | the substance is entirely in the gaseous phase
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| Why is the slope on water's triple point diagram negative? | The liquid phase is denser than the solid phase
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| What are supersaturated solutions? | When more solute can be dissolved in a solvent than is normal at that temperature. They are heated, and then rapidly cooled, and a slight disturbance can cause the solute to come out.
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| What is the difference between Molality and Molarity? | Molality is mol of solute per kg of solvent, so it is not dependent on temperature unlike molarity.
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| What are colligative properties? | They depend on the number of solute particles, not on the type of solute.
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| Explain vapor pressure lowering | When you add a solute to a solvent, the vapor pressure of the solution is lower than that of the pure solvent
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| Explain boiling point elevation | When you add a solute to a solvent, the boiling point is higher than that of the bp of the pure solvent
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| Explain freezing point depression | When you add a solute to a solvent, the freezing point is lower than that of the fp of the pure solvent
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| What is osmosis? | Osmosis the process by which water will diffuse out of a semipermeable membrane to achieve equilibrium.
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| What is osmotic pressure? | The pressure needed to stop osmosis
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| In the formula for calculating osmotic pressure, what does pi stand for? | Nothing, it's just a variable.
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| Why do unsaturated hydrocarbons undergo addition? | They are unsaturated, so a double or triple bond can break up to include other elements.
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| What do saturated hydrocarbons undergo? | Addition
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| Saponification is | when a base is added to a fat to make soap
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| Polymerization is | the linking of a hydrocarbon to form long chains of plastics
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| Esterification is | when an alcohol and carboxylic combine to form a great smelling ester
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| Fermentation produces | ethanol and carbon dioxide from sugar
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| Combustion involves | hydrocarbons reacting with oxygen to produce CO2 and H20
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| Cracking is | when large hydrocarbons are broken to form smaller ones
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| Memorize suffixes and functional groups |
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| What are isomers? | Isomers have the same formula, but they have different structures with different properties
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| What is the explicit formula for alkanes? | CxH2x+2
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| What is the explicit formula for alkenes? | CxH2x
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| What is the explicit formula for alkynes? | CxH2x
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| Organic chemistry is the study of | carbon and hydrogen containing compounds
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| What is the difference between cis and trans isomers? | On a cis isomer, the hydrogens are all on one side, and in a trans isomer, they are on opposite sides.
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| Alcohols with more than one hydroxide group are known as | dihydroxy alcohols or trihydroxy alcohols
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| In a series, what is the prefix to name the first of the series? The second of the series? | "Form" and "Ace" respectively
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| Amines have or don't have oxygen? | Amines don't have oxygen
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| Do amides have oxygen? | Yes, they do.
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| How do you know if an alcohol is primary, secondary, or tertiary? | Find the carbon to which the functional group is linked to. If the carbon is touching one other carbon, then it is a primary alcohol, if it is touching two others, it is a secondary alcohol, and three others would be a tertiary.
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