Chem Exam 4
Which of the following is the best Lewis Symbol for Oxygen?
O with 6 valence e- 2 on top and bottom 1 on each side
Obey's or violates octet rule? CS2 S=O=S 4e- on each s
Obeys
Polar covalent or Ionic? FeBr3
Polar Covalent
Polar covalent or ionic? CH4
Polar covalent
Polar covalent or ionic? SiCl4
Polar covalent
Determine which is the best insulator based on electronegativity values: a.) Na b.) Si c.) I
c.) I most electronegative from the choices
Which ionic compound would you expect to have the highest lattice energy? a.) KCl b.) RbCl c.) NaCl d.) LiCl
d.) LiCl
Polar covalent bonds are bonds between atoms whose electronegativites...
differ by less than 2 units Cl2O
Ionic bonds are bonds between atoms whose electronegativies...
differ by more than 2 units NaCl
What general trends in electronegativity occur in the periodic table?
electronegativity increases left to right and decreases down a group
Lattice energy correlates with ionization energy how?
if the distance is small then the charge is large, vice versa
Comparing atomic radius, in a group with the same number of electrons, the most negative ion is the ____________ and the most positive is the __________.
largest, smallest
Chp.5- Complete orbital diagram: Boron
1s^2, 2s^2, 2p^1
what is the electron configuration of N3-?
1s^2, 2s^2, 2p^6 [Ne] 2p^6 add 3 electrons to outermost shell because of -3
Chp.5- Complete orbital diagram Scandium(Sc)
1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^1
what is the electron configuration of Co2+?
1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^7 [Ar] 3d^7 lose 2 electrons because of +2
chp.6- what is the electron configuration of CO2+?
1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^7 [Ar] 3d^7 loses two electrons from lowest oribtal (4s) becuase of +2
what is the electron configuration of Ba2+?
1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 4p^6, 5s^2, 4d^10, 5p^6, 6s^2, [Xe] exclude the 6s^2 because of the +2
How many electrons can a single orbital hold?
2
How many resonance structures can be drawn for ozone, O3?
2
How many unpaired electrons are in the following elements? O= Si= K= As=
2 2 1 3
Chp. 5- Give orbital designations of electron with following quantum numbers: N=2, L=1, M1=1
2p
Rank orbitals from smallest to largest 3p, 5s, 4d, 2p
2p, 3p, 5s, 4d
Rank orbitals from smallest to largest 4s, 3d, 4p, 2s
2s, 4s, 3d, 4p
How many resonance structures are required in the electron-dot structure of (CO3)2-?
3
There is/are _____ unpaired electron(s) in the ground state configuration for Nitrogen
3
Rank the elements in decreasing order of first ionization energy according to element radius: Element X: 121 pm Element Y: 191 pm Element Z: 273 pm
Highest: Element X, Element Y, Element Z
Arrange the elements in decreasing order of first ionization energy: Ge, Se, In, Cs
Highest: Se, Ge, In, Cs
Polar covalent or ionic? CsBr
Ionic
Which bond? The nonmental atom gains one or more electrons
Ionic
Rank ions in order of decreasing radius: I-, Br-, Cl-, F-, At-
Largest: At-, I-, Br-, Cl-, F-
Classify each elements as a metal, nonmetal, or semimetal(metalloid.) Mg, Ne, S, As, Zn, Pb
Metal: Zn, Mg, Pb (low electronegativity) Nonmental: Ne, S (high electronegativity) Semimetal: As (intermediate electronegativity)
Rank from most to least electronegative: Phosphorus, Oxygen, Colbalt, and Potassium
Most: Oxygen, Phosphorus, Colbalt, and Potassium
fill in missing info: Na?SO4
Na2SO4
Which bond? There is a symmetrical electron distribution within the bond
Nonpolar covalent
Which element is stated in the electron configuration? 1+ ion: [Kr] 4d^10
Ag
Which element is stated in the electron configuration? 3+ ion: 1s^2, 2s^2, 2p^6
Aluminum (Al)
fill in missing info: Ba?(PO4)?
Ba3(PO4)2
Which metal in this list is most reactive? a.) lead b.) cesium c.) flourine d.) iron e.) silver
b
Which of the following is most likely solid at room temp? a.) H2S b.) Na2S c.) SO2
b.) Na2S becuase it is a metal
Which of the following compounds have the highest boiling point? a.) Br2 b.) NaBr c.) HBr d.) BrF
b.) NaBr ionic compounds have high boiling point
Chp.5- Which of the following is a valid set of 4 quantum numbers for a d electron in W? a.) n=6, l=2, ml=0, ms=−1/2 b.) n=6, l=2, ml=−3, ms=+1/2 c.) n=5, l=2, ml=−1, ms=+1/2 d.) n=5, l=1, ml=0, ms=+1/2
c
Which of the following has highest effective nuclear charge? a.) K b.) Si c.) Cl d.) Na
c
What is the formal charge on P in PCl5?
0
How many electrons should be shown in the Lewis structure for Hydrogen?
1
Rank orbitals from smallest to largest 4p, 4p, 6s, 3d
3d, 4p, 5p, 6s
Chp. 5- Give orbital designations of electron with following quantum numbers: N=3, L=0, M1=0
3s
According to Aufbau Principle, which orbital is filled before the following? 3p=_____ 4p=_____ 4f=______ 5d=______
3s 3d 6s 4f
Chp. 5- Give orbital designations of electron with following quantum numbers: N=4, L=2, M1=0
4d
Chp. 5- Give orbital designations of electron with following quantum numbers: N=4, L=3, M1=-2
4f
How many unpaired electrons are in Fe3+?
5
How many unpaired electrons are there in Fe3+?
5
In the best Lewis symbol for chlorine, how many valence electrons are there?
7
Chp.5- how many orbitals are in the 3rd state?
9
A certain element forms an ion with 18 electrons and a charge of 2+. What is the element?
Ca2+
Chp.7- Which of the following elements has the highest electronegativity? a.) P b.) Rb c.) Cl d.) Mg
Cl Electronegativity increases left to right and decreases top to bottom
Which bond? Electrons are not transferred completely between atoms
Covalent
Which element is stated in the electron configuration? 3+ ion: [Ar] 3d^3
Cr
What best describes an O3 molecule?
Each atom in ozone is connected to another atom by having a bond order of 1.5 (3/2)
Fill in missing info: Ga?(SO4)?
Ga2(SO4)3
Which element is stated in the electron configuration? 2+ ion: [Kr] 5s^2, 4d^10
Sn
Obey's or violates octet rule? BBr3 Br-B-B 6e- on Br
Violates
Electron Confriguration of [Ar] 3d^10 is?
Zn 2+
Chp.5- electron configuration for Arsenic (As)
[Ar] 4s^2, 3d^10, 4p^3
chp.5- electron configuration for bromide
[Ar] 4s^2, 3d^10, 4p^5
chp.5- electron configuration for nitrogen
[He] 2s^2, 2p^3
If the following elements were to form ions they would attain the same number of electrons as which nobel gas? Li, N, Mg, Ca, P, Rb, and Br
[He]- Li [Ne]- N, Mg [Ar]- Ca, P [Kr] Rb, br P and Br will gain electrons Li+ ion has 2 electrons, like He N3-, Mg2+ have 10 electrons, like Ne P3-, Ca2+ have 18 electrons, like Ar Br-, Rb+ have 36 electrons, like Kr
electron cofiguration for silver?
[Kr] 5s^1, 4d^10
chp.5- electron configuration for sulfur
[Ne] 3s^2, 3p^4
The compound ICl contains: a.) polar covalent bonds, with partial neg. charges on the Cl atoms b.) polar covalent bonds, with partial neg. charges on the I atoms c.) nonpolar covalent bonds d.) ionic bonds
a
What is the valence electron configuration for the element in Period 5, Group 3A? a.) 5s^2, 5p^1 b.) 3s^2, 3p^5 c.) 3s^2, 3p^3 d.) 5s^2, 5p^3
a
which group of ions is isoelectronic? (same number of electrons) a.) S2-, Ca2+, K+ b.) F-, Cl-, Br- c.) Rb+, Sr2+, Y3+
a & c
which has a larger ionization energy? a.) K or Br b.) S or Te c.) Ga or Se d.) Ne or Sr
a.) Br b.) S c.) Se d.) Ne
Which bond is more polar? a.) C-H or C-Cl b.) Si-Li or Si-Cl c.) N-Cl or N-Mg
a.) C-Cl b.) Si-Cl c.) N-Mg
An oxident is a substance that can accept the electrons from another reagent. Use electronegativity values to determine which of the following elements is a good oxidant? a.) Cl b.) Rb c) Co
a.) Cl Highest electronegativity
rank first ionization energies from largest to smallest: a.) Na, I, Cl b.) P, Sr, Mg c.) Ca, Se, Cs
a.) Cl, I, Na b.) P, Mg Sr c.) Se, Ca, Cs
Which of the following are radicles? a.) NO2 b.) Cl2 c.) C2H6 d.) CO2
a.) NO2 odd number of valence electrons (one not paired)
Which atom/ion would you expect to be larger in the following pairs? a.) O or O2- b.) Fe or Fe3+ c.) F or F-
a.) O2- b.) Fe c.) F-
Obey's or violates octet rule? PF5
violates; P can hold more than 8 electrons (F5= 10 e- on P)
Nonpolar covalent bonds (pure covalent) are bonds between atoms...
with the same or similar electronegativites H2
