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Directions on actual Exam: The exam consists of 2 sections (Chemical Bonding and Geometry and IMFs. Each multiple choice question is worth 4.33 points. You are allowed to use a scientific (nonprogrammable) calculator, periodic table, and VSEPR Theory Table.
Useful information:
H属rxn = 裡nD(bonds broken) - 裡nD(bonds formed)
where 裡n represents the sum of the moles of a particular type of bond
D represents bond energy per mole of bond
Chemical Bonding and Geometry
1.
The Lewis dot symbol for the calcium ion is
A)
2+
B)
Ca
C)
2+
D)
Ca2+
E)
Ca
2.
The electron dot structure for AsCl3 molecule shows
A)
a total of 84 electron dots
B)
three single bonds and 10 lone pairs
C)
two single bonds, one double bond, and 9 lone pairs
D)
one single bond, two double bonds, and 8 lone pairs
E)
three single bonds and one lone pair
3.
The correct Lewis structure for CO2 is: C
O
O
A)
O
O
B)
O
O
C)
O
O
D)
O
4.
Which of the following Lewis structures is incorrect?
A)
B)
C)
D)
E)
5.
How many covalent bonds will be formed by bromine in BrO3 for the dot structure that expands the octet to minimize formal charge and places negative formal charges on only the most electronegative atom(s). The Pauling electronegativity values are:
Br = 2.8; O = 3.5
A)
3
B)
4
C)
5
D)
6
E)
7
6.
Estimate the enthalpy change for the reaction 2CO + O2 2CO2 given the following bond energies.
BE(CO) = 1074 kJ/mol
BE(O=O) = 499 kJ/mol
BE(C=O) = 802 kJ/mol
A)
+2380 kJ/mol
B)
+744 kJ/mol
C)
+1949 kJ/mol
D)
561 kJ/mol
E)
744 kJ/mol
7.
Give the number of lone pairs around the central atom and the molecular shape of the ion ClO3.
A)
0 lone pairs, trigonal
B)
1 lone pair, bent
C)
1 lone pair, trigonal pyramidal
D)
2 lone pairs, T-shaped
E)
2 lone pairs, trigonal
8.
Which of the following substances is/are bent?
(i) H2S (ii). CO2 (iii) ClNO (iv) NH2 (v) O3
A)
only (iii)
B)
only (i) and (v)
C)
only (i), (iii), and (v)
D)
all are bent except for (iv)
E)
all are bent except for (ii)
9.
Which of the following molecules is polar?
A)
CH4
B)
SF6
C)
F2
D)
CH3F
E)
CO2
10.
Indicate the type of hybrid orbitals used by the central atom in TeF4.
A)
Sp
B)
sp2
C)
sp3
D)
sp3d
E)
sp3d2
11.
The hybridization of the O atom in CO2 will be
A)
S
B)
Sp
C)
sp2
D)
sp3
E)
sp3d
12.
The number of pi bonds in the molecule below is
A)
1
B)
2
C)
3
D)
5
E)
9
IMFs
13. Order the forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest .
a) dipole-dipole, London dispersion, ionic, and hydrogen-bonding
b) London dispersion, dipole-dipole, hydrogen-bonding, and ionic
c) hydrogen-bonding, dipole-dipole, London dispersion, and ionic
d) dipole-dipole, ionic, London dispersion, and hydrogen-bonding
e) London dispersion, ionic, dipole-dipole, and hydrogen-bonding
14. Which of the following would you expect to have the highest boiling point?
a) F2
b) Cl2
c) ...Course Name (Legal Political and Ethical Dimensions of Business)MG.docx
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Course Name (Legal Political and Ethical Dimensions of Business)MGMT520
Week 2: Assignment Instructions
In each week the learning assignment is designed to demonstrate your competence with the Terminal Course Objectives of the course. Prior to working on the assignment, you should read through the weeks chapters and lesson.
Clearly identify your work with your name, the date, the week number and the assignment name, and upload work to the Dropbox.
The questions are designed to probe the higher levels of thinking and learning such as analyzing, evaluating and creating, and so there often are no correct answers. Instead of focusing and who wins or loses the case, you should analyze, evaluate and create alternative solutions to the various issues presented while arguing and debating the connections between business, law, politics and ethics.
Terminal Course Objective: G
Case Study: International and World Trade Law - Counterfeiting
Write a 1-2 page reflective paper (double spaced) on the following questions while discussing the connections between business, law, politics and ethics.
One: There has been a movement in the last decade encouraging people to buy American. Discuss the legal and ethical issues related to boycotting goods from other countries. What are the practical business implications of such a move?
Two: The World Trade Organization, or WTO, is the largest and most influential of the trade organizations. China and other heavy counterfeiting nations are part of this group. What could WTO-participating nations do to address the problems of counterfeiting? What should they do?
Three: The United Nations Security Council, the main decision-making body at the UN, is comprised of five regular members: China, France, the Russian Federation, the United Kingdom and the United States. Ten more members are elected from the General Assembly. Given the make-up of the committee, what type of action might the UN take with regard to the counterfeiting issue?
Submit your assignment to the Dropbox.
揃 10165 - CHEM - 131 - Section 001 - Spring 2016 - General Chemistry Lec II
Top of Form
Question 1
Correct
Mark 3.00 out of 3.00
Flag question
Question text
All of the following are clues that a chemical reaction has taken place except
The reactant is smaller.
a.A flame occurs.
b.A color change occurs.
c. A solid forms.
Question 2
Question text
Balance the following equation in standard form and determine the sum of the coefficients.
a.6
b.4
c.3
d.14
e.7
Question 3
Question text
Balance this equation using the smallest possible integers, S + HNO3 H2SO4 + NO2 + H2O. What is the coefficient of water.
Select one:
a.2
b.6
c.8
d. 1
e.
Question 4
Question text
When the following equation is balanced using the smallest possible integers, what is the coefficent of oxygen gas?
C7H16(g) + O2(g) CO2(g) + H2O(g)
a.5
b.11
c.2
d.14
e.8
Question 5
Question text
True or false? The equation N2 + 3H2 2NH3 means that 1 g of N.STEM_GC11PC-If-31.pptx
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This document discusses chemical formulas and percent composition. It provides examples of calculating the percent composition of different compounds from their chemical formulas, such as NaCl, glucose, and Mg(OH)2. Empirical formulas can be determined from percent composition data by assuming 100 grams of the compound and calculating the moles of each element. Chemical equations are used to represent chemical reactions, and examples are given for writing and balancing equations. Common types of chemical reactions are also outlined.Chem 101 Spring 2017 Name _______________________________.docx
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Chem 101 / Spring 2017 Name: ______________________________________
Exam 2 // 198pts Lectures H through L (199)
1. Multiple Choice: Choose the best answer and put the number in the blank provided. (45pts)
A. _______ Compounds that have only non-metal element and only covalent bonds are
1. Didactic 2. Nobel Compounds 3. Ionic 4. Molecular
B._______ The Atomic Mass on the periodic table is:
1. The mass of the protons in an atom 2. The mass of a mole of atoms of a given element
3. The mass of an atom. 4. The Mass of a mole of protons
C._______ What is the major attractive force in a compound like NaCl?
1. Dipole-dipole, 2. London dispersion, 3. Ionic, 4. Hydrogen bonding
D. _______ Which of the following represents an Empirical Formula
1. N2O6 2. C6H12O6 3. C2H4 4. SO3
E. _______Atoms of the Non-metal elements generally form ions by
1. Losing electrons, forming positive ions 2. Losing electrons, forming negative ions
3. Gaining electrons, forming positive ions 4. Gaining electrons, forming negative ions
F. _______ The Atomic Mass Unit (AMU) is the mass of
1. A Mole of Carbon 2. A Hydrogen Atom 3. A Carbon Atom 4. An Electron
G. _______ A Polar Covalent bond has a
1. Random Charge 2. Positive Charge 3. Negative Charge 4. Dipole
H._______ Reaction ratios in gas phase reactions can be measured by
1. Temperature 2. Color 3. Volume 4. Time
I. ______ The formula showing the total number of each elements in a chemical formula is the
1. Molecular Formula 2. Atomic Formula 3. Thermodynamic Formula 4. Empirical Formula
J. ______ Which of the following would have the highest melting temperature?
1. H2O, 2. CO2 3. SO2 4. MgF2 5. NH3
K. ______ Carbon is very good at forming covalent bonds because
1. It is the best at forming Ionic Compounds 2. Its electronegativity is mid-range
3. Its electronegativity is very large 4. Its electronegativity is very small
L. ______ Ionic Compounds
1. Have poor solubility in water 2. Usually have low melting points
3. Conduct electricity when in solution 4. Readily form molecules
M. _____ The weakest of the intermolecular forces are:
1. Ionic 2. Covalent 3. Electron sea model 4. Dipole / Dipole 5. London
N. _____ Which statement is true about Hydrogen Bonds?
1. They are stronger than covalent bonds 2. They are the weakest of all interactions
3. They are stronger than ionic bonds 4. They are weaker then covalent bonds
O. _____ The physical properties of metals result from the inter-particle forces called:
1. Ionic 2. London 3. Electron sea model 4. Covalent 5. Dipole / Dipole
P. ______ Ionic compounds dissolve in water because the ions in the compound
1. Attract 2. Repel 3. Negate 4. Dissociate
/48
Chem 101 / Spring 2017 Name: ______________________________________
Exam 2 // 198pts Lectures H through L (199)
Q. ______ In the kinetic molecular theory gas particles are
1. Far apart 2 ...
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Directions: Please highlight or bold the correct answer.
1. Alkanes have the general formula,:
a. CnH2n4.
b. CnH2n2.
c. CnH2n.
d. CnH2n+2.
2. Alkenes have the general formula,:
a. CnH2n4.
b. CnH2n2.
c. CnH2n.
d. CnH2n+2.
3. Alkynes have the general formula,:
a. CnH2n4.
b. CnH2n2.
c. CnH2n.
d. CnH2n+2.
4. How many structural isomers are there of C4H10?
a. 4
b. 6
c. 2
d. 8
5. Which of these species is an aromatic compound?
a. C2H2
b. C6H12
c. C6H4Br2
d. C5H10
6. Which of these is the systematic name for the compound represented below?
a. 2-ethylbutane
b. 3-methylpentene
c. 3-methyl-1-pentene
d. 3-methyl-1-hexene
7. The group of atoms that is responsible for the characteristic properties of a family of organic compounds is called a(n):
a. reaction center.
b. functional group.
c. binding site.
d. enzyme.
8. Which one of the following functional groups is found in alcohols?
a. A
b. B
c. C
d. D
9. Which one of the following functional groups is found in carboxylic acids?
a. A
b. B
c. C
d. D
10. The reaction of an alcohol and a carboxylic acid yields a(n):
a. hydrocarbon.
b. ester.
c. ether.
d. aldehyde.
11. The reaction of Cl2 with CH4 to produce methyl chloride is an example of a(n):
a. free radical reaction.
b. addition reaction.
c. reduction reaction.
d. ester hydrolysis.
12. Which of these statements describes a condensation reaction?
a. Addition of H2O to a double bond
b. Linking an acid and an alcohol to make an ester and water
c. Addition of H2 to an alkene
d. Oxidation of ethanol to acetaldehyde
13. Bromination of benzene (C6H6), an aromatic compound,:
a. occurs by substitution rather than addition.
b. occurs by addition rather than substitution.
c. occurs more rapidly than bromination of a nonaromatic compound.
d. results in formation of 1,2,3,4,5,6-hexabromocyclohexane.
14. Which functional group, when present in a compound that is allowed to stand in air, poses a danger of slowly yielding explosive peroxides?
a. Ether
b. Alcohol
c. Carboxylic acid
d. Ketone
15. The molecule shown below is chiral; i.e., not superimposable on its mirror image.
a. True
b. False
16. The term, hybridization, refers to:
a. a change in the orbital configuration of electrons about an atom which has undergone bonding.
b. a way to describe elemental reactions.
c. changes in shapes of atoms.
d. a way to describe elements.
e. none of the choices apply.
17. When carbon atoms undergo bonding interactions,:
a. the hybridization of the atoms always changes.
b. the electronic state of the atoms change.
c. the reaction is always reversible.
d. none of the choices apply.
18. Enantiomers are:
a. sets of molecules with the same connectivity, atom to atom.
b. molecules with different orientation of substituents, about one or more atoms.
c. molecules which behave differently in biological systems.
d. non-super imposable mirror image isomers.
e. all of the choices apply.
19. Carbon chemistry is vastly diverse as ...Chemistry unit 9 presentation
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https://www.deped.gov.ph/wp-content/uploads/2019/01/General-Chemistry-1-and-2.pdf
General Chemistry
GenChem
STEM
Science, Technology, Engineering, and Mathematics
K to 12 Senior High School STEM Specialized Subject General Chemistry 1 and 2
Quarter 1 General Chemistry 1
Matter and Its Properties
Measurements
Atoms, Molecules and Ions
Stoichiometry
Percent Composition and Chemical Formulas
Chemical reactions and chemical equations
Mass Relationships in Chemical Reactions
Gases
Daltons Law of partial pressures
Gas stoichiometry
Kinetic molecular theory of gases
Quarter 2 General Chemistry 1
Electronic Structure of Atoms
Electronic Structure and Periodicity
Chemical Bonding
Organic compounds
Quarter 3 General Chemistry 2
Intermolecular Forces and Liquids and Solids
Physical Properties of Solutions
Thermochemistry
Chemical Kinetics
Quarter 4 General Chemistry 2
Chemical Thermodynamics
Chemical Equilibrium
Acid-Base Equilibria and Salt Equilibria
ElectrochemistryScience and technology 111
Science and technology 111Maritess Bonsato
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This document contains a 30-item multiple choice science and technology exam covering chemistry concepts such as balancing chemical equations, classifying reaction types, calculating molar mass, and gas laws. The questions assess understanding of topics like coefficients, subscripts, moles, empirical formulas, vapor pressure, kinetic energy, and boiling points. The correct answers are not provided.Dr. Burke Practice Test 2
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This document contains a practice test for Exam 2 covering Chapters 3, 4, and 7 of a chemistry course. The test has 30 multiple choice questions testing concepts like balancing chemical equations, stoichiometry, gas laws, solution concentrations, acid-base reactions, and periodic trends. The key is provided with the letter answers for each question.
Formulating Clear Statement of Research Problem WEEK 2.pptx
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Inquiry, Investigations and Immersion WEEK 2 lessonGP2-4th WEEK DLL-4th.docx
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This document is a daily lesson log for a Grade 11 physics class taught by Mary Ann I. Santos. Over four class periods, the students learned about geometric optics concepts including the laws of reflection and refraction, total internal reflection, and applications involving ray optics experiments. The lessons involved reviewing concepts, presenting examples, discussing new skills like solving context-rich problems, and evaluating student learning through activities and problems. Formative assessments were given to check student understanding of key ideas like Malus' law governing the transmission of light through polarizers. The log included reflections on teaching strategies, student performance, and areas for improvement.GP2-3rd WEEK DLL-4th.docx
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The document is a daily lesson log for a Grade 11 physics class. It outlines the objectives, content, learning resources, and procedures for four class periods on the topics of:
1) Alternating current, LC circuits and their applications (Day 1)
2) Electric charge, Coulomb's law, and electric fields and flux (Day 2)
3) Reflection, refraction, total internal reflection, and applications of geometric optics (Day 3)
4) Reflection, refraction, dispersion, and polarization (Day 4)
The log provides details on the standards, competencies, examples, group activities, and concepts that will be discussed to teach the physics principles for each day.GP2-2nd WEEK DLL-4th.docx
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The document is a daily lesson log for a Grade 11 physics class. It summarizes the objectives, content, learning resources, and procedures for four class sessions on topics including LC circuits, electric charge, electric fields, and electromagnetic waves. The objectives are for students to understand concepts like inductance, capacitance, Coulomb's law, and properties of waves. Class activities include reviewing concepts, analyzing examples, group problem-solving, and quantitative discussions to reinforce understanding.More Related Content
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Module 8 Check Your Understanding 1
Directions: Please highlight or bold the correct answer.
1. Alkanes have the general formula,:
a. CnH2n4.
b. CnH2n2.
c. CnH2n.
d. CnH2n+2.
2. Alkenes have the general formula,:
a. CnH2n4.
b. CnH2n2.
c. CnH2n.
d. CnH2n+2.
3. Alkynes have the general formula,:
a. CnH2n4.
b. CnH2n2.
c. CnH2n.
d. CnH2n+2.
4. How many structural isomers are there of C4H10?
a. 4
b. 6
c. 2
d. 8
5. Which of these species is an aromatic compound?
a. C2H2
b. C6H12
c. C6H4Br2
d. C5H10
6. Which of these is the systematic name for the compound represented below?
a. 2-ethylbutane
b. 3-methylpentene
c. 3-methyl-1-pentene
d. 3-methyl-1-hexene
7. The group of atoms that is responsible for the characteristic properties of a family of organic compounds is called a(n):
a. reaction center.
b. functional group.
c. binding site.
d. enzyme.
8. Which one of the following functional groups is found in alcohols?
a. A
b. B
c. C
d. D
9. Which one of the following functional groups is found in carboxylic acids?
a. A
b. B
c. C
d. D
10. The reaction of an alcohol and a carboxylic acid yields a(n):
a. hydrocarbon.
b. ester.
c. ether.
d. aldehyde.
11. The reaction of Cl2 with CH4 to produce methyl chloride is an example of a(n):
a. free radical reaction.
b. addition reaction.
c. reduction reaction.
d. ester hydrolysis.
12. Which of these statements describes a condensation reaction?
a. Addition of H2O to a double bond
b. Linking an acid and an alcohol to make an ester and water
c. Addition of H2 to an alkene
d. Oxidation of ethanol to acetaldehyde
13. Bromination of benzene (C6H6), an aromatic compound,:
a. occurs by substitution rather than addition.
b. occurs by addition rather than substitution.
c. occurs more rapidly than bromination of a nonaromatic compound.
d. results in formation of 1,2,3,4,5,6-hexabromocyclohexane.
14. Which functional group, when present in a compound that is allowed to stand in air, poses a danger of slowly yielding explosive peroxides?
a. Ether
b. Alcohol
c. Carboxylic acid
d. Ketone
15. The molecule shown below is chiral; i.e., not superimposable on its mirror image.
a. True
b. False
16. The term, hybridization, refers to:
a. a change in the orbital configuration of electrons about an atom which has undergone bonding.
b. a way to describe elemental reactions.
c. changes in shapes of atoms.
d. a way to describe elements.
e. none of the choices apply.
17. When carbon atoms undergo bonding interactions,:
a. the hybridization of the atoms always changes.
b. the electronic state of the atoms change.
c. the reaction is always reversible.
d. none of the choices apply.
18. Enantiomers are:
a. sets of molecules with the same connectivity, atom to atom.
b. molecules with different orientation of substituents, about one or more atoms.
c. molecules which behave differently in biological systems.
d. non-super imposable mirror image isomers.
e. all of the choices apply.
19. Carbon chemistry is vastly diverse as ...Chemistry unit 9 presentation
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油
This document consists of a chemistry exam with multiple choice questions covering various topics in chemistry including the periodic table, chemical bonding, reactions, and organic chemistry. It provides instructions for students to answer 40 multiple choice questions in 45 minutes by choosing the correct answer and recording it on an answer sheet. A copy of the periodic table is provided for reference.Terminal test
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This document contains a 33 question multiple choice chemistry test covering various topics in general, organic, and inorganic chemistry. The questions assess knowledge of atomic structure, chemical bonding, stoichiometry, acid-base chemistry, and the naming and properties of organic compounds including alkanes, alkenes, alcohols, ketones, aldehydes, carboxylic acids, esters, and amines.M.Sc.I Inorganic Chemistry Question paper
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This document discusses atomic mass and isotopes. It begins by explaining that an atomic mass unit (amu) is used to discuss the mass of atoms, where 1 amu is 1/12 the mass of a carbon-12 atom. Atomic masses listed in the periodic table are in amu. Isotopes have different atomic masses that result in the average atomic mass not being a whole number. Examples are provided to demonstrate calculating average atomic masses from the masses and abundances of isotopes.SHS STEM General Chemistry MCT 9. Organic Compounds
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https://www.deped.gov.ph/wp-content/uploads/2019/01/General-Chemistry-1-and-2.pdf
General Chemistry
GenChem
STEM
Science, Technology, Engineering, and Mathematics
K to 12 Senior High School STEM Specialized Subject General Chemistry 1 and 2
Quarter 1 General Chemistry 1
Matter and Its Properties
Measurements
Atoms, Molecules and Ions
Stoichiometry
Percent Composition and Chemical Formulas
Chemical reactions and chemical equations
Mass Relationships in Chemical Reactions
Gases
Daltons Law of partial pressures
Gas stoichiometry
Kinetic molecular theory of gases
Quarter 2 General Chemistry 1
Electronic Structure of Atoms
Electronic Structure and Periodicity
Chemical Bonding
Organic compounds
Quarter 3 General Chemistry 2
Intermolecular Forces and Liquids and Solids
Physical Properties of Solutions
Thermochemistry
Chemical Kinetics
Quarter 4 General Chemistry 2
Chemical Thermodynamics
Chemical Equilibrium
Acid-Base Equilibria and Salt Equilibria
ElectrochemistryScience and technology 111
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This document contains a 30-item multiple choice science and technology exam covering chemistry concepts such as balancing chemical equations, classifying reaction types, calculating molar mass, and gas laws. The questions assess understanding of topics like coefficients, subscripts, moles, empirical formulas, vapor pressure, kinetic energy, and boiling points. The correct answers are not provided.Dr. Burke Practice Test 2
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This document contains a practice test for Exam 2 covering Chapters 3, 4, and 7 of a chemistry course. The test has 30 multiple choice questions testing concepts like balancing chemical equations, stoichiometry, gas laws, solution concentrations, acid-base reactions, and periodic trends. The key is provided with the letter answers for each question.More from maryannsantos32 (9)
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AC current efficiently transfers over long distances, providing more power using rotating magnets that cause electrons to flow directionally at frequencies of 50-60Hz, changing direction forward and backward. It is produced by generators and has impedance as its passive parameter with a power factor between 0 and 1, including sinusoidal, trapezoidal, triangular, and square wave forms. DC current loses power over long distances with steady magnetism causing electrons to flow in one direction at zero frequency, moving steadily forward. It is produced by cells or batteries and has resistance as its only passive parameter with a power factor always of 1, including pure and pulsating forms.Recently uploaded (20)
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Reviewer in general chemistry lesson 1 and 2
- 2. 1. Which of the following characteristics best describes a SOLID? A.It has no definite shape B.It has definite shape and volume C.It has definite shape and no definite volume D.It has definite volume and no definite shape
- 3. 2. Two atoms, 127Hg and 131Hg are isotopes because they have the same number of ______ but different numbers of neutrons. A. atomic number C. atomic weight B. electrons D. protons
- 4. 3. Which of the following formulas represents a molecular compound? A. Xe C. H2O2 B. HO D. CH2O
- 5. 4. If the lines in the structural formula shows the bonding of the elements in a compound, how many bonds do two lines in a structural formula indicate? A. double C. single B. lone pair D. triple
- 6. 5. Name the covalent compound: C6F8
- 7. 6. 3.5 mol of He g
- 8. 7. 40 g of O no. of O atoms
- 9. 8. Calculate the molar mass of NH3
- 10. 9. Calculate the molar mass of C2F2Cl4.6H2O
- 11. 10. Balance the chemical equation: C2H5OH + O2 CO2 + H2
- 12. 11. A balloon filled with He gas has a volume of 4.0x10^3 at 23C. What volume will the balloon occupy at 50C?
- 13. 12. A compound is found to consist of 43.64% Phosphorus and 56.36% Oxygen. The molar mass of the compound is 283.88 g/mol. What is the empirical formula of the compound? (P = 30.97, O = 16) A. PO2 C. P205 B. P204 D. P4010
- 14. 13. Before performing an experiment Mateo calculated that the reaction of 20.7 grams of CaCO3 will produce 11.59 grams CaO. After performing the experiment, he found out that only 6.81 grams of CaO was produced. Calculate the success rate of the experiment. A. 58% C. 58. 76% B. 58. 50% D. 59%
- 15. 14. In the reaction 2H2 + O2 2H2O, what is the mole ratio of oxygen to water? A. 2: 1 C. 1: 4 B. 8: 1 D. 1: 2
- 16. 15. In building bicycle, you need 2 wheels, bicycle frame, seat and a handle bar. How many bicycles can be made in 16 wheels, 10 seats, 9 frames, and 10 handle bars. Given the available parts, which of the following is/are set as the limiting reactant/s? A. bicycle frames C. seats B. handle bars D. wheels
- 17. 16. Daltons Partial Pressure can be calculated by using which of the following? A. molar mass C. mole conversion B. mole fraction D. mass percentage
- 18. 17. Assume that excess CuO reacts with 5.6 L H2 at STP according to the following equation: CuO + H2 Cu + H2O, what will be the mole value? A. 22.4 mol C. 0.56 mol B. 5.6 mol D. 0.25 mol
- 19. 18. Relationship of volume and pressure in Boyles Law?
- 20. 19. Value of constant in Ideal Gas Law?
- 21. 20. How to compute partial pressure?