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Give the charge that would be on each of the following atoms if ionized. Ba     [ba] I        [i] Ag    [ag] CuI  [cui] O      [o] Rb     [rb] P       [p] OH   [oh] Cr (IV)  [criv] H         [h]  

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Using the electronegativity table and the rules (which suggest that a difference in electronegativity below 0.4 is equally shared, 0.5–1.7 is polar covalent, and greater than 1.8 is ionic), the bonds in BeBr2 (the electronegativity of Be is 1.5 and Br is 2.8) would be classified as ________.

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Name the following compounds: Fe2O3 FeCl2 Na2S Al2O3   Name of A: [iron3oxide]     Name of B: [iron2chloride] Name of C: [Sodiumsulfide]     Name of D: [aluminumOxide]        

On this heating curve for water, do the following: Explain why there are the flat plateaus labeled melting and boiling. Using your knowledge of the molecular structure of water and of intermolecular forces, explain why the plateau is greater for boiling than for melting. Submit your response using the text editing tools in the box below. See the description for details “The image shows a heating curve for a substance, plotting temperature (in °C) against the heat absorbed. The graph indicates the phases of matter as the substance is heated: Solid: The substance is in a solid state at temperatures below 0°C. Melting: At 0°C, the substance begins to melt, transitioning from solid to liquid. Liquid: After melting, the substance remains in liquid form as the temperature rises. Boiling: At around 100°C, the substance starts to boil, transitioning from liquid to gas. Gas: The substance eventually reaches a gaseous state as the temperature exceeds 100°C.”

The number of calories in 3.0 g of glucose (blood sugar) is listed as 10.0 cal. If 15.0 g of glucose is reacted in a calorimeter, such that all of the energy is released and captured in a 1,000.00-gram water bath surrounding the calorimeter, what is the expected final temperature of the water following the reaction if the initial water temperature is 21.0 °C? The specific heat of water is 4.18 J/g °C or 1.00 cal/g °C. Work out the problem on a separate piece of paper and upload a photo of your response at the end of the test. Please mark the problem clearly and show your work. Enter your answer in the text box below.

Answer the following questions using the simplified solubility rules below: Cations that are always soluble: Compounds of group 1 cations (Na+, K+, etc.) and ammonium (NH4+) are always soluble. Anions that are always soluble: Nitrate (NO3−) anions are always soluble. Halides: Compounds of the halides (Cl−, Br−, I−) are soluble except for silver(I) (Ag+) and lead(II) (Pb2+). Sulfate: Compounds of sulfate (SO4 2−) are soluble except for group 2 cations (Ca2+, Sr2+, Ba2+) and lead(II) (Pb2+). Everything else: Most other compounds not listed as soluble in rules 1–4 are assumed to be insoluble.

The boiling point of CH4 is −162 °C and the boiling point of CCl4 is 77 °C. Identify the principal intermolecular forces in each of these compounds and briefly explain the large difference in boiling points. Submit your response using the text editing tools in the box below.