CHE 131 Lecture Notes - Lecture 13: Covalent Bond, Equivalence Point, Single Displacement Reaction

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cerisegiraffe538

2 Nov 2017

School

Stony Brook University

Department

Chemistry

Course

CHE 131

Professor

Benjamin Hsaio, Jiangyong Jia, Roy Lacey

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CHE 131 Full Course Notes

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Oxidation-reduction(redox) is the net movement of electrons from one reactant to another. There is a shift of electrons rather than a full transfer, therefore ions do not form. This type of reaction involves the transfer of electrons. Metals high on the list react more easily with cold water than metals low on the list. Metals become less reactive the farther down the series you go. A metal higher up in the list will displace the ions of another metal farther down the list from solution. Metals participate in two types of single displacement reactions. A reactive metals can displace h 2 metal can also displace the ion of a less reactive metal from solution. At the equivalence point of a redox titration the number of electrons lost by the oxidized species is equal to the number of electrons gained by the reduced species. Electrons moves as nonpolar covalent bonds are replaced by polar covalent bonds.

Related Questions

Please help question 1-6 please, Thank you!

1. The valence electrons are located in the ____________ orbitals of an atom.

2. Positive ions are formed by the ____ of electrons, while negative ions are formed by the ____ of electrons.

Identify the charge of the metal ion in each of the following

- A. B. C. D. E. F. G. H. I. J.	Al₂S₃
- A. B. C. D. E. F. G. H. I. J.	CoSO₄
- A. B. C. D. E. F. G. H. I. J.	AgCl
- A. B. C. D. E. F. G. H. I. J.	VS₃
- A. B. C. D. E. F. G. H. I. J.	NiO
- A. B. C. D. E. F. G. H. I. J.	Mn₃(PO₄)₅

A.	+3
B.	+2
C.	+1
D.	+6
E.	+5
F.	+7
G.	-1
H.	-2
I.	+4
J.	-3

4. Electrons are shared in covalent compounds so that each atom has ____ electrons which satisfies the _____ rule.

5. The names of covalent compounds use _____ to state the nuber of atoms which is dervived from the _____ names. For example, 2 atoms would be identified as _____

Polyatomic ions are ions that contain more than one ____________ in its formula.

	A.	atom
	B.	molecule
	C.	electron
	D.	ion

1)The NaCl2 ionic salt does not exist. Which of the followingstatements best explains why?

A. Because the formation of Na2+ is an unfavorable process due tothe great amount of energy required to remove the 2nd electron fromthe Na atom (the 2nd electron would have to be removed from thecore electrons of the Na atom).
B. Because the Cl- anion is too large for there to be two of themattached to one Na+ ion.
C. Because NaCl2 is actually a polyatomic ion with a -1 charge, andnot an ionic salt. In the presence of another Na+ ion, the Na2Cl2salt would form.
D. Because Cl2 has no charge and therefore would not be attractedelectrostatically to the positively charged Na2+ cation.

2)Select the false statement below.

A. The first ionization energy of an atom is smaller than thesecond ionization energy of the same atom.
B. Phosphorus has a greater first ionization energy than magnesium,and the reason for this is because P has a greater effectivenuclear charge (Zeff) than Mg.
C. The following process is an endothermic process and representsthe first ionization energy of an atom A:A(g) ? A1+(g) + e1-
D. Fluorine has a greater first ionization energy than iodine, andthe reason for this is because fluorine has a greater amount ofshielding of outer electrons by inner electrons than doesiodine.

3)The Group 5A elements N,P,As have lower (less negative) electronaffinities than most of the Group 4A or Group 6A elements becauseN,P,As have half-filled subshells.

True
False

4)A fluorine atom is smaller than a bromine atom, and a potassiumatom is larger than a lithium atom.

True
False

5)A certain main-group element exhibits the following successiveionization energies in kJ/mol:

IE1 = 100; IE2 = 1200; IE3 = 2300; IE4 = 3100; IE5 = 4200

Select the false statement about this element below.

A. This is likely a Group 1A element.
B. This element is typically found uncombined in nature (that is,it is not usually found in compounds, but rather as a freeelement).
C. If this element is given a symbol of "J", it would form an ioniccompound with sulfur as J2S.
D. If this element was in period 2 of the periodic table, it wouldbe lithium.

6)Select the false statement below.

A. Generally speaking, non-metallic elements have greater effectivenuclear charge (Zeff) than metallic elements in the sameperiod.
B. Generally speaking, as you go down a group in the periodictable, there is successively greater shielding of the outer-shellelectrons by the inner-shell electrons.
C. Generally speaking, the heavier alkali metals can be predictedto exhibit greater shielding of the outer-shell electrons by theinner-shell electrons than lighter alkali metals.
D. Generally speaking, as you go across a period in the periodictable, the effective nuclear charge (Zeff) decreases because eachsuccessive element contains more protons in the nucleus than theprevious element and the outer electrons are all in the same shellas you go across a period.

7)Place the following in order of increasing size:

O2-, F1-, Li1+

A. F1- < Li1+ < O2-
B. Li1+ < O2- < F1-
C. Li1+ < F1- < O2-
D. F1- < O2- < Li1+

8)Select the false statement below.

A. The following set of quantum numbers is allowed:
n = 4, l = 2, ml = -2, ms = +1/2
B. The n = 1 shell of any given atom can accomodate up to 2electrons.
C. The n = 4 shell of any given atom can accomodate up to 16electrons.
D. In any given atom, the l = 2 subshell can accomodate up to 5electrons that have negative spins (ms =

redgoldfish403

1.An inorganic base dissociates in water into ?a)one or more hydrogen ions and one or more anions b)one or more hydroxide ions and one or more reactions c)one or more hydrogen ions and one or more captions d)one or more hydroxide ions and one or more anions 2.An atom becomes a cation by? a)accepting electrons into its outermost electron shell b)giving up electrons from its outermost electron shell c)donating protons to another atom d)accepting proton from another atom 3.An atom of oxygen has 8 protons ,8electroenes and 8 neutrons.How would you expect the electrons to be arranged in this atom? a)all electrons are located in the nucleus of the atom b)all 8 electrons are located in the outermost electron shell c)all 8 electrons are located in the electron shell nearest the nucleus d)2 electrons are in the electron shell nearest the nucleus and 6 are in the second shell 4.Which solution is acidic? a) H2O b)H2O+ NA(+) +OH(-) c) H20+H(+) +Cl (-) d)Na(+) + HCO3 (-) 5.which of the following is true about the products of the chemical reaction?a) in the synthesis reaction , the products contain the fewer atoms than the reactants b) in the synthesis reaction , the products contain more atoms than the reactants c)in any chemical reaction the products may contain more or fewer atoms than the rectants because the reaction is a random event d)the products of chemical reactions always contain the same number of atoms as the reactants 6.Can you choose which thing is not like others ? a)lactose b)maltose c)sucrose d )fructose 7Which of the following is not organic compound? a)CO2 b)H2O c)CH2O d)NH3 8.Which of the following is a lipid ? a)C6H12O6 b)C22H44COOH c)C2H4NH2 d)CO2 9.Which of the following does not dissolve readily in a water? a)proteins b) amino Acids c) steroids d) Carbohydrates 10.Which of the following is organic asid? a)H2CO3 b)NaOH c)HCL d)KCL 11.Nitrogen is the element important to the composition of ? a)carbohydrate b)proteins and nucleis acids c)fats d)glycerol 12.Which of the following is protein ? a)sucrose b) cholesterol c)raffinose d)mannose 13.In the formation of a polymer , dehydration synthesis occurs between ? a) the amino groups of 2 different amino acids b)the acid groups of two different amino acids c)the amino group of one amino acid and the acid group of the other d)all of the above

CHE 131 Lecture Notes - Lecture 13: Covalent Bond, Equivalence Point, Single Displacement Reaction

CHE 131 Full Course Notes

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