Docsity
Log inSign up
Docsity
Prepare for your exams
Prepare for your exams

Study with the several resources on Docsity

Earn points to download
Earn points to download

Earn points by helping other students or get them with a premium plan

Guidelines and tips
Guidelines and tips
Sell on Docsity
Sell on Docsity
Log inSign up

Prepare for your exams

Study with the several resources on Docsity

Find documents

Prepare for your exams with the study notes shared by other students like you on Docsity

Search Store documents

The best documents sold by students who completed their studies

Search through all study resources
Docsity AINEW

Summarize your documents, ask them questions, convert them into quizzes and concept maps

Explore questions

Clear up your doubts by reading the answers to questions asked by your fellow students

Earn points to download

Earn points by helping other students or get them with a premium plan

Share documents
download point icon20 Points

For each uploaded document

Answer questions
download point icon5 Points

For each given answer (max 1 per day)

All the ways to get free points
Get points immediately

Choose a premium plan with all the points you need

Study Opportunities

Choose your next study program

Get in touch with the best universities in the world. Search through thousands of universities and official partners

Community

Ask the community

Ask the community for help and clear up your study doubts

University Rankings

Discover the best universities in your country according to Docsity users

Free resources

Our save-the-student-ebooks!

Download our free guides on studying techniques, anxiety management strategies, and thesis advice from Docsity tutors

From our blog

Exams and Study
Go to the blog

Chem 1160 Final Exam Study Guide With Complete Solutions., Exams of Chemistry

Stanford UniversityChemistry

Chem 1160 Final Exam Study Guide With Complete Solutions.

Typology: Exams

2024/2025

Available from 07/14/2025

joyce-williams
joyce-williams 🇺🇸

2.8K documents

1 / 22

Toggle sidebar

This page cannot be seen from the preview

Don't miss anything!

bg1
Chem 1160 Final Exam Study Guide With
Complete Solutions
Exam 1 questions 1 - 20 - answer
1) consider the question: is there any active force between a pencil in the earth? Is this a
scientific question?
I. Yes
II. No
BECAUSE
III. It can be tested an answered through observations and experiments.
IV. The answer is already known and we find it online.
V. There is no way to design an experiment to answer this question. - answer C. II and IV
2) which of the following properties ascribed to atoms by Dalton do we still considered
valid?
I. Elements are composed of small indivisible, indestructible particles called atoms.
II. All atoms of an element are identical and have the same mass and properties.
III. Adams of a given element are different from atoms of other elements.
IV. compounds are formed by the combinations of atoms of two or more elements. -
answer D. III and IV
3) electrons are negatively charged. Which experiment provided evidence to support this
claim? What is the specific evidence used to support this claim?
EXPERIMENT:
I. The gold foil experiment.
II. The cathode ray experiment.
EVIDENCE:
pf3
pf4
pf5
pf8
pf9
pfa
pfd
pfe
pff
pf12
pf13
pf14
pf15
pf16

Partial preview of the text

Download Chem 1160 Final Exam Study Guide With Complete Solutions. and more Exams Chemistry in PDF only on Docsity!

Chem 1160 Final Exam Study Guide With

Complete Solutions

Exam 1 questions 1 - 20 - answer

  1. consider the question: is there any active force between a pencil in the earth? Is this a scientific question? I. Yes II. No BECAUSE III. It can be tested an answered through observations and experiments. IV. The answer is already known and we find it online. V. There is no way to design an experiment to answer this question. - answer C. II and IV
  2. which of the following properties ascribed to atoms by Dalton do we still considered valid? I. Elements are composed of small indivisible, indestructible particles called atoms. II. All atoms of an element are identical and have the same mass and properties. III. Adams of a given element are different from atoms of other elements. IV. compounds are formed by the combinations of atoms of two or more elements. - answer D. III and IV
  3. electrons are negatively charged. Which experiment provided evidence to support this claim? What is the specific evidence used to support this claim? EXPERIMENT: I. The gold foil experiment. II. The cathode ray experiment. EVIDENCE:

III. Most of the positively charged alpha particles shot at I thin gold foil past straight through. IV. A small fraction of the positively charged alpha particle shot at a single foil were deflected. V. The beam of particles emitted from the cathode bent towards the positively charged plate. VI. The beam of particles emitted from the cathode behaved the same no matter what type of metal the cathode was made of. - answer D. II and VI

  1. which of the following contain(s) atoms? A. Heat B. Light C. Energy D. Dust E. All of them. - answer D. Dust
  2. which of the following represent molecules that are compounds? - answer C. II and III. (The colorectal images are two boxes, one filled with 3 pairs of 3 circles, unfilled, and the second box with 3 pairs of 2 circles filled in.)
  3. The diagram below shows alpha particles being fired at a piece of gold foil. Where will the majority of the alpha particles be detected (Point I, II, or III) and why? - answer D) III. and VI - The alpha particles go straight through the atom, because it is the most empty space.
  4. Thompson's cathode ray tube experiment provided false what part of Dalton's atomic theory? A. All atoms are indivisible and indestructible. B. All atoms of a given element are identical. C. All matter is made of atoms. D. Compounds are formed from the combination of two or more elements.

C. Because the repulsive force, between the overlapping electron clouds, is dominant. D. Because there is more potential energy and kinetic energy when the atoms are close together. - answer B. Because electrostatic attractive force, from the instantaneous dipoles, is dominant.

  1. Bromine (Br) melts at 266K and boils at 332K. Which of the following is the best representation of bromine at 300 K? - answer C. (Think of a box and inside the box there are multiple oval shapes with two nucleus loosely stacked together.
  2. The diagram to the right is fortwo subatomic particles. What does the curve show. (The diagram is a potential energy diagram with the curve going down). I. The potential energy decreases as the objects get closer together. II. The potential energy increases as the objects get closer together. WHICH TWO SUBATOMIC PARTICLES COULD THIS CURVE REPRESENT? III. Two neutrons IV. Two electrons V. One proton and one electron - answer C. I and IV
  3. which statement best describes the forces that exist between helium atoms in a solid state? A. The electron cloud on one helium atom is attracted to the electron cloud on the other atom. B. The nucleus of one helium atom is repelled by the nucleus of the neighboring atom. C. The helium atoms share electrons, forming a bond. D. The partial positive ends of one atoms instantaneous dipole attracts the partial negative end of the neighboring Atoms induced dipole. E. Both atoms have mass, so they are attracted to each other by gravitational forces. - answer B. The nucleus of one helium atom is repelled by the nucleus of the neighboring atom.
  4. wanna covalent bond is formed between two nitrogen atoms:

I. Energy is absorbed. II. Energy is released. III. A molecule is formed. IV. The nitrogen changes from the gaseous to liquid state. - answer E. All the above

  1. The London dispersion force between two neon atoms compared to the London dispersion force between two argon atoms where both systems are the most stable is: I. The same. II. stronger. III. weaker. BECAUSE IV. They are both noble gases. V. Neon has a smaller electron cloud, therefore there will only be smaller separation of change resulting in a weaker force. VI. Neon has a smaller electron cloud, therefore there will be a larger separation of charge resulting in a stronger force. - answer D. III and V
  2. is the following statement true or false? When chlorine freezes, London dispersion forces are formed. The statement is: I. True II. False BECAUSE III. When a substance freezes, covalent bonds are formed. IV. there are LDFs in both the solid-state and the liquid state, but more in the solid-state. V. There are LDFs in the solid-state, but not in the liquid state. - answer B. I and V
  3. which do you predict to have the higher boiling point, di - fluorine (F2) or neon (Ne) and why? (Imagine fluorine has a larger electron cloud).
  1. The potential energy curves for two substances are shown to the right one curve represents two atoms interacting through a London dispersion force on the other curve represents two atoms forming a covalent bond. (Imagine a potential energy diagram with one solid line that dips down further than a dotted line)
  • which curve represents the atoms that form a covalent bond? A. The solid long because the atoms are further apart when the covalent bond forms. B. The solid line because it takes more energy to separate the atoms. C. The dotted line because the atoms are closer together when the covalent bond forms. D. The dotted line because it takes less energy to separate the atoms. - answer C. The dotted line because the atoms are closer together when the covalent bond forms. Exam 2 questions 1 - 20 - answer
  1. select the evidence and reasoning that supports the claim that light is a wave. EVIDENCE I. II. III. REASONING IV. V. VI. - answer C. II and V Question 2 was crossed out from this exam. - answer
  1. The energies of four photons of light are listed below which photon has the longest wave length? E= h c/lambda A. E= 1 x 10^ -12 J B. E= 8x10^ -16 J C. E= 5 x 10^ -18 J D. E= 2 x 10^ -19 J - answer D. E= 2 x 10^ -19 J
  2. The diagram to the right shows what happens when orange light shines on a piece of metal. Which of the diagrams below best illustrates what happens when higher intensity orange light shines on the same piece of metal. (The image is hv with an arrow pointing to a piece of metal). - answer D. Two hv arrows being absorbed into the metal.
  3. what is the evidence that supports the claim that light as a particle? A. Wood light shines through a double slit, the light produces an interference pattern. B. Increasing the amplitude makes light appear brighter. C. When light shines on metal there is a threshold frequency, below which no electrons are ejected from a metal. D. Electrons produce an interference pattern. E. Electrons absorb certain photons of light to move to higher energy levels. The electrons can omit the photon to move back to the lower energy level. - answer C. When light shines on metal there is a threshold frequency, below which no electrons are ejected from a metal.
  4. An MRI (magnetic resonance imaging) Machine operates at a frequency of 30 kilohertz (kHz), what wavelength radiation does this correspond to?

II. The valence electrons have different energies. III. The valence electrons are in different types of orbitals. IV. The valence electrons are in different size orbitals. - answer E. II and IV

  1. what is the electron configuration of Mg+? A. 1S^2 2S^2 2P^6 3S^ B. 1S^2 2S^2 2P^6 3S C. 1S^2 2S^2 2P^ D. 1S^2 2S^2 2P^ E. 1S^2 2S^2 2P^6 3S^2 3P^3 - answer B. 1S^2 2S^2 2P^6 3S^
  2. consider K+ and Cl-. Which do you predict is larger and why? A. K+ is larger because potassium is farther to the left and further down the periodic table than chlorine. B. K+ is larger because it contains more electrons so there are more electron - electron repulsions. C. K+ and Cl- are the same size because they both contain the same number of electrons so there is the same amount of electron - electron repulsion. D. Cl- is larger because anions are always larger than cations. E. Cl- is larger because fewer protons are attracting the same number of electrons as in K+.
  • answer E. Cl- is larger because fewer protons are attracting the same number of electrons as in K+.
  1. Use the data table for the first eight ionization energies of a particular element shown below to predict and explain the element you would expect to show this trend in successive ionization energies.

I. Fluorine II. Oxygen BECAUSE III. Core electrons are more strongly attracted to the nucleus than valence electrons. IV. Balance electrons release more energy when they are removed from the atom. - answer C. II and III

  1. not including recently man - made elements, which graph best represents how the number of elements in the universe has changed over time? (Think of a line graph with a sharp incline and then stables out into a straight line). - answer B.
  2. atomic radius _____ from left to right across a row on the periodic table. I. Increases II. Decreases BECAUSE III. The number of electrons increases IV. The mass increases V. The relative attraction between the protons and the outer electrons increases. - answer E. II and V
  3. how many quarantines electrons does one atom of iodine (I) have? A. 36 core and 17 valance. B. 7core and 36 valence. C. 36 core and 7valence. D. 46 core and 7 valence. - answer D. 46 core and 7 valence.
  1. according to the Heisenberg uncertainty principle, is it impossible to know precisely both a position and the _____ of an electron. A. Mass B. Color C. Momentum D. Shape - answer C. Momentum
  2. The atomic radius of a main - group elements in the periodic table generally increases down a group because _____. A. Effective nuclear charge increases down a group. B. Effective nuclear charge decreases down a group. C. The principal quantum number of the valence electrons increases. D. Both, effective nuclear charge and the principal quantum number of valence electrons increases down a group. - answer C. The principal quantum number of the valence electrons increases. Exam 3 questions 1 - 24 - answer
  3. to the right is a complete molecular orbital diagram for a diatomic molecule. The electrons are shown in the atomic orbitals in the molecular orbitals. How many bonds exist between the atoms in the diatomic molecule? A. 0 bonds B. 1 bond C. 2 bonds D. 3 bonds

E. 4 bonds - answer C. 2 bonds

  1. carbon can exist in many forms known as allotropes. To search allotropes are diamond and graphite. Unlike diamond, graphite conducts electricity. This is because... A. In graphite, there are hybrid orbitals used for bonding that contain electrons. B. In graphite, all the electrons are in Sigma bonsai loud conduct Tiffany of electricity through these bombs. C. And graphite, there are on hybridized P - orbitals that extend over the entire sheet forming a delocalized Pi bonding network where electrons are free to move. D. And graphite, the bonding electrons do not have enough energy to move and can therefore conduct electricity. - answer C. And graphite, they're on hybridized P - orbitals that extend over the entire sheet forming a delocalized Pi bonding Netwerk where electrons are free to move.
  2. what is the best explanation for why metals are ductile? A. Valence electrons carry charge anywhere within molecular orbitals that span the metal. B. Photons are absorbed in reemitted. C. Metallic bonds involve delocalized electrons whereas covalent bonds involve localized electrons. D. Valence electrons act as a sea of electrons, surrounding the nuclei and holding them together. - answer B. Photons are absorbed and reemitted.
  3. compare the two molecular representations shown to the right. THESE STRUCTURES REPRESENT I. The same molecule. II. Isomers. III. Different molecules that are not isomers.

A. London dispersion forces B. London dispersion forces and covalent bonds C. London dispersion forces and hydrogen bonds D. London dispersion forces, hydrogen bonds, and covalent bonds E. Covalent bonds - answer A. London dispersion forces

  1. for the structure to the right, what is the electron center geometry for the oxygen atom that the arrow is pointing to? A. Linear B. Bent C. Tetrahedral D. Trigonometry planar E. Trigonal pyramid - answer C. Tetrahedral
  2. use the Lewis structure in question eight to answer this question. What is the shape around the oxygen atom that the air was pointing to? A. Linear B. Bent C. Tetrahedral D. Trigonal planar E. Trigonal pyramid - answer B. Bent
  3. to Lewis structures are shown below. Are these molecules the same or are they isomers? I. same

II. Isomers BECAUSE III. They have the same formula but different atom connectivity IV. They have the same formula and same atom connectivity V. They have different numbers of C a d H atoms - answer A. I and III

  1. The Lewis structure for ethane (C2H4) is shown below. What is the hybridization in the shape around the carbon labeled with the arrow? A. Sp^3 and tetrahedral B. Sp^2 and tetrahedral C. Sp^3 and linear D. Sp^2 and trigonal planar E. Sp^2 and trigonal pyramid - answer A. Sp^3 and tetrahedral
  2. The Lewis structure for ethane (C2H4) is shown in question 11. which statements below are true regarding ethanes Pi bond? I. The PI bond and everything is made from the interaction between an and hybridized P orbital on each carbon atom II. The PI bond in ethane is made from the direct orbital overlap between the Sp^2 hybrid orbitals on each carbon atom. III. Rotating around the PI bond and everything requires energy to break the interaction. IV. There is free rotation around the PI bonding ethane. - answer A. I and III
  3. dipole - dipole interactions in London dispersion forces are two types of intermolecular forces. For molecules of about the same size... A. London dispersion forces are the stronger force due to the temporary, fluctuating
  1. Three molecules of methanol (CH3OH) are shown below. Which of the labeled interactions are hydrogen bonding interactions. A. I B. II C. II and III D. IV E. I, II, III - answer D. IV
  2. what are the strongest intermolecular forces present in dimethyl ether (CH3OCH3) in the liquid state? A. London dispersion forces interactions. B. Dipole - dipole interactions. C. Hydrogen bonding. D. Covalent bonds. - answer B. Dipole- dipole interactions.
  3. True or false, NaBr has the lowest melting point of the following ionic compounds: NaBr, CaO, LiF, and MgO. I. True II. False BECAUSE III. NaBr is least ionic IV. NaBr Is made of larger ions with smaller charges V. NaBr is made of smaller ions with smaller charges - answer C. I and IV
  1. what is the most likely formula for the compound formed in calcium and fluorine? A. CaF B. Ca2F C. CaF D. Ca2F3 - answer A. CaF
  2. if the same amount of thermal energy were transferred to equal masses of water, copper, granite, and ethanol, which substance would reach the highest temperature? A. Water (Cs= 4.18 J/g °C) B. Copper (Cs= 0.385 J/g °C) C. Granite (Cs= 0.79 J/g °C) D. Ethanol (Cs= 2.42 J/g °C) E. They would all reach the same temperature since an equal amount of thermal energy is transferred to an equal mass of each. - answer B. Copper
  3. what happens on the molecular level when thermal energy is added to increase the temperature of water from 10°C to 50°C? A. The kinetic energy of water molecules increases, making the molecules collide more forcefully with a thermometer. This forces the mercury of the capillary tube causing an increase in the temperature scale. B. The water molecule speed up, and collide with the thermometer, transferring energy to the thermometer. This energy causes the mercury atoms and the thermometer to vibrate more, and the liquid expands - thus showing an increase in the temperature scale. C. The water molecules expand until some of the bonds holding the atoms together break. D. The water molecules move faster and bump into each other. This bumping causes friction in which Causes heat consequently, the water temperature rises. - answer A. The kinetic energy of water molecules increases, making the molecules collide more forcefully