1,3 Propanediol, HOCH2CH2CH2OH can form intra H bonds and inter molecular H bonds. Draw the structure of 1,3 Prop. that shows an intramolecular H bond. What does the 1,3 mean?
Hi, I need assistance with the following questions: The electron configuration of the S2- ion is _______. a. [Kr]3s23p-6 b. [Ne]3s23p2 c. [Ar]3s23p2 d. [Ar]3s23p6 e. [Ne]3s23p6 Of the compounds below, _____ has the smallest ionic separation. a. SrBr2 b. KF c. RbCl d. Rbf e. K2S Given the electronegativities b
The basis of the VSEPR model of molecular bonding is ____________. a. regions of electron density on an atom will organize themselves so as to maximize s-character b. atomic orbitals of the bonding atoms must overlap for a bond to form c. hybrid orbitals will form as necessary to,
Both my mum and I have looked everywhere and cannot find what I need. I have to find the alcohol formulas for; Methanol, Ethanol, Propanol, Butanol, Pentanol, Hexanol, Heptanol and Octanol. We have found chemical tables and compounds but not specifically any containing alcohol. Please can you help or tell me where i could loo
Please help with the following questions. Question 6 The formula CH3CH2CH2=CH2 represents an alkene an alkyne an alcohol benzene Question 7 The number of orbitals in a d subshell is: 1 2 3 5 7 Question 8 _____ is credited with the modern structure of the
Please help with the following problem. Question 1 All acids have the common component H+, true or false? Question 2 Calculate the number of moles of aluminum in 96.7g of Al. a) 0.28 b) 3.6 c) 7.4 d) 4.2 Question 3 The melting point of bromine is -7°C. What is this in °F? a) -12.6°F b) -28
Molecule: [:O triple bond C single bond N (3 pairs electrons)] What are the formal charges on these atoms? With which formula can the formal charge be calculated?
For each molecule, draw the Lewis structure first, then apply the VSEPR model according to the following rules: 1. Count the number of electron pairs around the central atom (both bonding pairs and unshared pairs). Treat double and triple bonds as if they were single bonds. 2. Refer to the table given below to predict the geom
How can you know that HNO3 is nitric acid and HNO2 is nitrous acid? I need to understand this difference between acids.
I need to write an essay that explains how a given set of names for binary ionic and molecular compounds can be determined. For an example let's pick KF which is potassium flouride. How can that name be found? I also need to discuss the nomenclature and chemical formulas in this essay by distinguishing between them. Wh
The problem to solve is to formulate in which way two carbon atoms are described by using atomic orbitals. First one has to find out the electronic structure of a carbon atom by locating this element in the periodic table. Second step is then to fill the orbitals with the given number of electrons using Hund's rule. The third
What do each of the "items" stand for in the following formula for ethyl cyanoacrylate? CN l H2C=C l COOC2H5
4.81 Which of these aqueous solutions would you expect to be the best conductor of electricity at 25° C? Explain your answer? (a) 0.20M NaCl (b) 0.60M CH3COOH (c) 0.25M HCl (d) 0.20M Mg (NO3)2
6 ) Iron has a density of 7.86 g/cm3. The volume occupied by 55.85 g of iron is: 7 ) Which pair of elements would be most likely to form an ionic compound? P and Br Cu and K C and O O and Zn Al and Rb 8 ) Which is the formula for the binary compound of potassium and nitrogen? KN K2N NK2
Write the formula for the compound rubidium nitrite.
I have been given the attached as a balanced chemical equation for the complete oxidation of one mole of oleic acid. 2CH3(CH2)7CH = CH(CH2)7COOH + 51)2 = 36CO2 = 36CO2 + 34H20 Using the following table how do I work out the energy released by the reaction? TYPE OF BOND AVERAGE ENERGY CONTENT/kJ mol-1 Single ca
This is a past exam for practice. Please complete question 5 only. 20 5. Write brief notes on any four of the following: a. Metal-organic vapor phase epitaxy b. Berry's rotation. c. Effect of polarization on melting points d. IR spectroscopy as a tool for structure determination of inorganic compounds e. Rochow pr
3. Explain why: a. Lewis acid strengths of boron halides are in the order BBr3 >> BCl3 > BF3 opposite to the order expected based on electronegativities. b. Radius ratio rule is correct only 66% of the times in predicting coordination numbers in ionic compounds. c. Me3B is a monomer, whereas Me3Al exits as a dimer. d. Vis
1. Explain the following, with suitable examples: a. Frontier orbitals b. A 3-center 2e- bond c. Tendency of P to form d pi -p pi bond d. Self dissociation of ammonia e. Formation of halogen cation **Please see attachment for proper citation of symbols.
Out of 250 questions, I am unsure of the following: 1.For a given substance that exhibits liquid-crystalline properties, the transition from solid to liquid-crystal state occurs: a.over a range of temperatures that includes the melting point of the soild. b. at a well defined temperture above the melting point of the solid.
Using the table of bond energies to determine the DH for the reaction: 2H--F(g) H--H(g)+ F--F(g).
Why do square planar geometries occur in d7, d8, and d9 ions with strong field- pi acceptor ligands, except in cases in which ligand geometry requires it?
How is it possible that [Co(h20)6]3+ will oxidize water but [Co(Nh36]3+ is stable in aqueous solution? Both are mondentate ligands. I thought the proximity of the nitrogens after one has bonded to the cobalt would make it more likely to react, because the entropy would be lowered. They are also both low spin complexes.
My professor gave us this and told us that some of these problems will be on our test. I just want to make sure I know how to do all of them correctly. Thanks! 1. When describing structures of solids, especially ionic solids, structure types are typically associated with the structures of well-known species. If a system we
In forming a covalent bond, electrons are (a) shared by two atoms (b) given up by an atom (c) taken up by an atom (d) none of the above (e) all of the above
Please give a complete MO description of the molecule HF.
The alkali metal hexachloroplatinates: Na2[PtCl6], K2[PtCl6], Rb2[PtCl6], Cs2[PtCl6] have the same type of lattice structure. How would you expect the solubility of these salts to vary (increase or decrease) from the sodium salt to the cesium salt? Explain your answer.
Please give complete answers and details on how to think about these problems. Also, explain reasoning on how you get your answer please! Predict the signs of q and w for the following: A. Condensing water in an exothermic process at P=1 atm and T=370K. H20(g) -> H20(l) B. Subliming CO2(dry ice) - an endothermic pro
7 general chemistry questions. Example: The reaction of silver metal and dilute nitric acid proceeds according to the equation above. If 0.10 mole of powdered silver is added to 10 milliliters of 6.0-molar nitric acid, the number of moles of NO gas that can be formed is: (a) 0.015 mole (b) 0.020 mole (c) 0.030 mole (d) 0
6 general chemistry questions - i.e. "Atoms of an element, X, have the electronic configuration shown above. The compound most likely to form with magnesium, Mg, is: (a) MgX (b) Mg2X (c) MgX2 (d) Mg2X3 (e) Mg3X2 " *(Please see attachment for complete equations and problems)