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Chem 145 exam 3

QuestionAnswer
Write the balanced equation of the formation of aluminum oxide (Al2O3) from aluminum being exposed to oxygen gas. 4 Al + 3 O2 = 2 Al2O3
Name an element likely to be oxidized. Most metals and H2
Of the following, which is the best reducing agent: Cl2, H+, (SO4)2-, Mg Mg - the reducing agent is the element that is oxidized in a redox reaction
Of the following, which is the best oxidizing agent: Cl2, H2, (SO4)2-, Mg Cl2 - the oxidizing agent is the element that is reduced in the redox reaction
The oxidation number for N in (NO3)1- is.... +5
The oxidation number for P in (PO4)3- is... +5
Is the following a redox reaction: Cu + 2 Ag+ = 2 Ag + (Cu)2+ Yes - The Ag is reduced (gaining electrons) and Cu is oxidized (losing electrons)
Is the following a redox reaction: CH4 + 2 O2 = CO2 + 2 H2O Yes - The O is reduced and the reducing agent is H
Is the following a redox reaction: SiCl4 + 2 H2O = 4 HCl + SiO2 No - no element was oxidized or reduced. All kept their original oxidation number
What is the overall balanced neutralization reaction that would result in the formation of the salt calcium sulfate (CaSO4) Ca(OH)2 + H2SO4 = CaSO4 + 2 H2O
What is the balanced equation for the reaction between aqueous Na2SO4 and aqueous Pb(NO3)2 Na2SO4 + Pb(NO3)2 = PbSO4 + 2 NaNO3
What is the net ionic equation of Na2SO4 + Pb(NO3)2 = PbSO4 + 2 NaNO3 (Pb)2+ + (SO4)2- = PbSO4 **Remember to show the charges on the ions!
"(NO3)2 = PbSO4 + 2 NaNO3 Na+ and (NO3)- **Remember to show the charges on the ions!
What classification is the equation Na2SO4 + Pb(NO3)2 = PbSO4 + 2 NaNO3 exchange reaction
What is the balanced reaction for the formation of copper (I) oxide from its elements 4 Cu + O2 = 2 Cu2O
When would you take the time to use formal charges? What is it helpful in deciding? You use formal charge when a molecule has resonance forms. It helps decide which resonance form is most likely possible.
What must a molecule have to have a "pi bond"? What are "the players/entities/things" involved directly when a "pi bond" is in place (what's doing what with what to create this bond)? A pi bond is the second bond between atoms when there needs to be 2 pairs of shared electrons. Py and Pz shells create the "pi bond"
In order to have a molecule with a molecular geometry of "square planar", how many electron groupings must be about the central atom? 6
Name two possible molecular geometries for a central atom that has hybridization of sp2. Triangular planar and bent
Which of the following have cis- and trans-isomers: ClBrC=CH2 or ClHC=CHBr ClHC=CHBr
The most electronegative atom of the following: C, N, Si, P N
Name two possible molecular geometries for a central atom that has hybridizations of d2sp3 Square pyramidal and square
For the molecule CCl2F2 (where "C" is the central atom), which atoms has, or atoms have a partial negative charge? F and Cl
Lis a molecule compound that contains a non-polar covalent bond CO2, CH4
In order to have a molecule with a molecular geometry of "T-shaped", how many electron groupings must be about the central atoms? 5
List ALL of the following elements that can form compounds with five or six pairs of valence electrons surrounding their atoms out of: C, P, O, F, Cl, B, Se, I P, Cl, Se, I
Name and element that has very high electronegativity F - Fluorine
Why does Fluorine have a very high electronegativity? Because it is so small and the shared pairs have very small space (very limited shielding) from the nucleus
When an element is said to have high electronegativity what does that mean? That the element is the most polar in the molecule and will pull other electron pairs towards itself
For each molecule of carbon monoxide, which atom has a partial plus charge? Carbon
Name a compound that contains polar covalent bonds. H2O
The most electronegative out of the following: C, N, Si, P N
Of the following single bonds, which is the most polar: C-C, C-O, C-Cl, C-F, C-N C-F
Of the following single bonds, which is the least polar: C-C, C-O, C-Cl, C-F, C-N C-C
The S-C-S bond angle in a CS2 molecule is predicted to be _______ degrees 80
Why are ionic compounds solids at room temperature? They have a very strong bond/attraction of each other and are held very tightly together
Why are most polar molecules liquids? The atoms have a partial plus and partical negatives creating a static cling - they tend to be sticky
Why are most non-polar molecules gases? There is very little attraction between atoms - they move around very freely
Created by: juret7674
 

 



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