silica(a common stationary phase) has Si-OH(silanol) groups on the surface which readily form hydrogen bonds with solutes. Does silica have a greater affinity for polar or non-polar compound?
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silica(a common stationary phase) has Si-OH(silanol) groups on the surface which readily form hydrogen bonds with solutes. Does silica have a greater affinity for polar or non-polar compound?
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- ● Explain why higher average kinetic energy results in higher vapor pressure in terms of IMFs.Why is water an excellent solvent for most ionic compounds and polar covalent molecules, but not for non-polar compounds?Explain each of these properties of water, and describe how each is conferred by the dipolar nature of a water molecule: high specific heat capacity; high heat of vaporization; unique density behavior; high surface tension; capacity to be a good solvent for ions of salts.
- Given the information below, calculate the lattice enthalpy for MX(s), where M is a group 1 metal, and X is a group 17 element (standard state: X2(g)). ΔfH°(MX) = -462 kJ mol−1 ΔsubH°(M) = 127 kJ mol−1 D(X2) = 442 kJ mol−1 IE1(M) = 480 kJ mol−1 Eeg1(X) = -142 kJ mol−1 Express your answer to four significant figures. ΔlattH°(MX) = Answer kJ mol−1Is iodine monochloride in solid form conductive with respect to electrical conductivity? Why or why not?List at least two properties of water and describe why it exhibits such in terms of its molecular structure and bonding behavior.
- Minerals that generally form from the evaporation of a water-based solution belong to which chemical group?How many of these elements would be able to bond with the silica tetrahedra SiO4 - molecules? Group of answer choices are A = 4 B = 2 c = 1 Match it to the correct element. Na+ (sodium) Mg2 + (magnesium) Fe 2 + (iron) Fe 3 + (iron) Al 3 + (aluminum) Ca 2 + (calcium) K+ (potassium) |explain why the mobility on an ion might increase with ionic radius even though the mobility is defined as u=ze/6pina, where a is the radius. Assume all other variables are constant
- Aspirin has a higher molar mass compared to salicylic acid, however aspirin melts at a lower temperature than salicylic acid. Provide a brief explanation for this observation. Table 1 Compound: Formula: Salicylic Acid C;H6O3 Aspirin C9H3O4 Molar Mass: 138.12 Melting point: Ka 158-160°C 1.08 x 10³ 180.15 140-142°C 2.72 x 10$ pKa Solubility (g/100ML) 2.99 4.57 0.18 0.25Explain implications of the hydrogen bonding between water molecules The images to the right depict hydrogen bonding between water molecules. What are some effects of these bonding forces? HS+ H 8+ 4....... 8- (Η) O H 8+ Hydrogen bonds OH- O 8- Ho+ https://www.scienceabc.com/pure-sciences/is-carbon-dioxide-co2-polar-or-nonpolar.html; https://socratic.org/questions/why-does-water-form-hydrogen-bonds-1Coulombs Law describes the interaction between two charges and varies by the magnitude of these charges and inversely with the distance between them. For atoms, we'll label the charges as the nuclear charge and electron charge. 9192 9nuclelec As you go up in atomic number (Z), the number of protons in the nucleus increases, making the charge on the nucleus increase, so that in general. qnuc = Z ·(+1) However if we think only of the electrons in the outermost shells (valence electrons), they do not see the full strength of the nuclear charge because it is partially shielded (or canceled out if you prefer) by the core electrons. So we define something called effective charge. Shielding Experiences net charge of about 1+ Nucleus Effective Charge = # of protons Zeff = Z – core # of core electrons In general, Zeff increases as you go across in the periodic table. 1. Fill out the following table to verify that effective charge increases as you go across a row. Element Na Mg Al Si P S CI Ar…
