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CHEM 121 Midterm: Practice Questions

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24 Jan 2019

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The average mass of a boron atom is 10. 81. 10. 81% greater than 50: for which of the following compounds does 1. 0 g represent 5. 55 10-2 mol, no2, h2o, nh3, c2h6, no, the mass of 0. 82 mol of a diatomic molecule is 131. 3 g. identify the molecule. I2: nahco3 is the active ingredient in baking soda. How many grams of oxygen are in 0. 32 g of. 0. 18 g: compound x2y is 60% x by mass. Which % value below is closest to the actual percent y by mass of the compound x2y2. 80: an oxybromate compound, nabrox, where x is a whole number, is analyzed and found to contain. 4: the empirical formula of a group of compounds is chcl. Lindane, a powerful insecticide, is a member of this group. 8: when the equation c10h22 + o2 co2 + h2o is balanced with the smallest set of integers, the sum of the coefficients is.

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Related Questions

use this vocabulary to fill in the blank. charge- a vacuum- small volume - atom- mass - nucleus- angle of defection- oil drop - mass to charge ratio- smaller particle - protons- electron- magnetic and electric fields- gold foil - neutrons-empty space-Thomson used --------to measure the -----of a cathode ray particle.Thomson's experiments are important because they showed that the-------------- is clearly composed of----------. The Milikan -------experiment is important because it determined the -----of an ---------.Using Thomson's ---------and Milikan's----------- the -----of an --------- was determined.Rutherofrd's ----------experiment is important because it clearly demonstrated that the ----------- is mostly-----------.Rutherford's results also showed that the most of atom's ---------------is located in the -------which has a very -------------.

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 =