CHEMISTRY COMMUNITY

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Do you all think that grades will be adjusted this quarter or is the average too high?

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Does anybody have any tips for calming down so I can think straight during the final?

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Do we have access to any test banks so we can practice some more?

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How do you find if something is a stronger base?

6C.17 Which is the stronger base, the hypobromite ion, BrO2, or morphine, C17H19O3N? Justify your answer.

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How do you write formulas for conjugate acids?

6A.1 Write the formulas of the conjugate acids of (a) CH3NH2, methylamine; (b) NH2NH2, hydrazine; (c) HCO3-; and the conjugate bases of (d) HCO3-; (e) C6H5OH, phenol; (f) CH3COOH

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How do you know if a ligand can be polydentate?

9C.5 Which of the following ligands can be polydentate? If the ligand can be polydentate, give the maximum number of places on the ligand that can bind simultaneously to a single metal center: (a) HN(CH2CH2NH2)2; (b) CO322; (c) H2O; (d) oxalate.

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Can someone do part A as an example? 9C.3 Use the information in Table 9C.1 to write the formula for each of the following coordination compounds: (a) potassium hexacyanidochromate(III) (b) pentaamminesulfatocobalt(III) chloride (c) tetraamminediaquacobalt(III) bromide (d) sodium bisoxalato(diaqua)f...

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Can someone help me out with this question?

9C.1 Name each of the following complex ions and identify the oxidation number of the metal: (a) [Fe(CN)6]4-; (b) [Co(NH3)6]3+; (c) [Co(CN)5(OH2)]2-; (d) [Co(NH3)5(SO4)]+.

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What are the different shapes of coordination compounds?

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What are the rules for naming coordination compounds?

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Can someone help me with this problem?

2F.9 Identify the hybrid orbitals used by the phosphorus atom in each of the following species: (a) PCl41; (b) PCl62; (c) PCl5; (d) PCl3.

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Can someone walk me through this problem?

2F.17 Describe the structure of the formaldehyde molecule, CH2O, in terms of hybrid orbitals, bond angles, and s- and p-bonds. The C atom is the central atom to which the other three atoms are attached.

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What are the shapes with lone pairs?

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What are all of the possible molecular shapes there can be?

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What is test 2 supposed to cover?

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How do you find the hybridization?

2F.5 State the hybridization of the atom in boldface red type in each of the following molecules and ions: (a) BeCl2; (b) BH3; (c) BH42; (d) SiF4.

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How do you do problems like this?

2F.1 State the relative orientations of each of the following hybrid orbitals: (a) sp3; (b) sp; (c) sp3d2; (d) sp2.

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How do you know when a molecule is polar or nonpolar? What are the differences? 2E.27 Predict whether each of the following molecules is likely to be polar or nonpolar: (a) C5H5N (pyridine, a molecule like benzene except that one OCHO group is replaced by a nitrogen atom); (b) C2H6 (ethane); (c) CHC...

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How do you find the bond angles like in these questions?

2E.17 Predict the bond angles at the central atom of the following molecules and ions: (a) ozone, O3; (b) azide ion, N32; (c) cyanate ion, CNO2; (d) hydronium ion, H3O1.

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Does anyone have any recommendations for youtube channels that can I can refer to if I need help with any topics I have trouble with in this class?

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How are Lewis Structures different for inorganic, organic, and biological compounds?

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Can someone help me out with this question?

2C.11 Draw the Lewis structure and state the number of lone pairs on xenon, the central atom of each of the following mole- cules: (a) XeOF2; (b) XeF4; (c) XeOF4.

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What are different factors that affect covalent bond lengths?

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How do you draw resonance structures?

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How do I find bond length with covalent radii?

2D.19 Use the covalent radii in Fig. 2D.11 to calculate the bond lengths in the following molecules. Account for the trends in your calculated values: (a) CF4; (b) SiF4; (c) SnF4.

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How do you find bond length?

2D.13 Place the following molecules or ions in order of decreas- ing bond length: (a) the CO bond in CO, CO2, CO322; (b) the SO bond in SO2, SO3, SO322; (c) the CN bond in HCN, CH2NH, CH3NH2. Explain your reasoning.

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Can someone help me out with this please?

2D.1 Place the following elements in order of increasing electro-
negativity: antimony, tin, selenium, and indium.

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How do you know if species are radicals?

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How do you find the number of valence electrons in an element?

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Can someone give me a quick summary on drawing lewis structures?

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The unit is meters, but can also be a variation of that like nano- and pico- meters

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E=hv measures the energy of a photon, while E=1/2mv^2 measures kinetic energy.

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It basically says that an orbital can only have a max of 2 electrons, and that 2 electrons can't have the same sign.

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Can somebody help me out and give a quick summary of how you find an electron configuration by doing it for one of the atoms in 1E-11?

Write the ground-state electron configuration for each of the following atoms: (a) sodium; (b) silicon; (c) chlorine; (d) rubidium.

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Can somebody explain how you find angular momentum quantum numbers like in this question?

What are the principal and orbital angular momentum quantum numbers for each of the following orbitals: (a) 6p; (b) 3d; (c) 2p; (d) 5f?

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Can someone explain to me the difference between wave-like and particle-like properties?

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When you know the wavelength you can find the frequency by using the formula λ v = c, where v is the frequency (nu) and c is a constant for the speed of light. Once you find the frequency you can use the equation f (aka nu) = velocity/λ . I hope this helps!

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The way I did this problem was by using the equation: λ v = c, where v is the frequency and c is a constant for the speed of light. That number that you saw is "c." I hope this helps!

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Molarity is the moles of solute per liter of the solution and molality is the moles of solute per kilogram of the solvent. Thank you to Khan Academy for educating us :)

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I believe that he will be posting more as we go through the material.

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