What is the dissolution reaction of Zn(NO3)2 and Sr(NO3)2? Solution . All chlori

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. All chlorides, bromides, and iodides are soluble except those containing Ag^+, Pb^2+, or Hg2^2+. 4. All sulfates are soluble except those containing Hg2^2+, Pb^2+, Sr^2+, Ca^2+, or Ba^2+. 5. All hydroxides are insoluble except compounds of the alkali metals, Ca^2+, Sr^2+, and Ba^2+. 6. All compounds containing PO4^3-, S^2-, CO3^2-, and SO32- ions are insoluble except those that also contain alkali metals or NH4^+. Reactivity series (http://en.wikipedia.org/wiki/Reactivity_… are used to determine the products of single displacement reactions, whereby metal A will replace another metal B in a solution if A is higher in the series. A metal can replace metals listed below it in the activity series, but not above. 1. a strip of since is placed in a solution of silver nitrate. (Zn + AgNO3 ----> ?) A: Zn + 2AgNO3 --> Zn(NO3)2 + 2Ag (single displacement reaction) (no precipitate) 2. a solution of coppter (2) nitrate is spilled onto a sheet of aluminum. (very slow reaction but does occur) A: Cu(NO3)2 + Al --> Al(NO3)3 + Cu (single displacement reaction) (no precipitate) Aluminium is above Copper in the reactivity series, but copper does not react vigorously and quickly with chemicals , thus slow reaction . 3. a solution of acetic acid is added to a solution of sodium hydroxide. A: CH3COOH + NaOH --> CH3COO^-Na^+ + H2O (acid base reaction) (salt is formed =>CH3COO^-Na^+) out of the molecules CO, CO2, O2, HF, and F2...which has the largest dipole moment? A: The Bond Dipole is two atoms in a bond, such that the electronegativity of one atom changes and draws the electrons towards the other, causing a partial negative charge. There is an increase difference in polarity, and an increase in dipole. The answer is HF electronegativity (F) = 3.98 (Pauling scale) electronegativity (F) = 2.1 (Pauling scale) Difference in electronegativity (H-F) = 3.98-2.1 Difference in electronegativity (H-F) = 1.88 (Pauling scale) There are large differences in electronegativity between hydrogen and fluorine, so that the majority of electron density in the hydrogen-fluorine bond ends up on the much more electronegative fluorine. Bonds such as this in which the electrons are not shared evenly are referred to as polar covalent bonds. Polar covalent bonds have a bond dipole moment. e.g. CO2 CAN'T be the answer; Carbon dioxide has two polar covalent C-O bonds. However, the bond dipole moments exactly cancel each other since they are pointing in exactly opposite directions. Thus, CO2 has no molecular dipole moment. Please note that the cancellation of bond dipole moments does not change the existence or placement of electron density. Each individual C-O bond has the normal bond dipole moment even though the molecular dipole moment is zero. By the way, you should be able to identify the carbon atom in CO2 as being sp hybridized.

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