Copy and Edit

Exam 2

Description

Conceptual physical science
Kimberly Lopez
Quiz by Kimberly Lopez, updated more than 1 year ago
Kimberly Lopez
Created by Kimberly Lopez almost 8 years ago
357
0
0

Resource summary

Question 1

Question
What is the valence shell?
Answer
  • It is the shell of electrons in element V (atomic no. = 23)
  • It is the shell of electrons in an atom that is the least reactive.
  • It is the outermost shell of electrons in an atom.
  • It is the same as the orbital configuration
  • It is the last partially filled orbital in an atom.

Question 2

Question
Which of the following best describes ionic bonding?
Answer
  • two atoms exchanging a set of electrons
  • two atoms sharing a set of electrons
  • one atom giving up some of its electrons to another atom
  • when two elements with same charge are held together by electrostatic forces
  • none of the above

Question 3

Question
How many valence electrons does bromine (Br, atomic no. = 35) have?
Answer
  • 28
  • 7
  • 21
  • 1
  • 35

Question 4

Question
The source of an atom's electronegativity is the
Answer
  • kinetic energy electrons have orbiting the nucleus.
  • repulsive force occurring among electrons within the same shell.
  • repulsive force occurring between electrons within neighboring shells.
  • positively charged atomic nucleus.

Question 5

Question
Metals are often used for making designer jewelry because they
Answer
  • conduct electricity
  • do not conduct heat well
  • are shiny
  • are strong but can be bent
  • c and d (are shiny, are strong but can be bent)

Question 6

Question
Which of the following is the main form of intermolecular attractions among water molecules?
Answer
  • hydrogen bonding
  • induced dipole-induced dipole
  • polar-induced polar
  • ion-dipole
  • covalent bonding

Question 7

Question
If a neutral atom gains two electrons, what is the electrical charge of the atom?
Answer
  • +1
  • +2
  • neutral
  • -1
  • -2

Question 8

Question
What is the difference between a dipole-dipole interaction and an ion-dipole interaction?
Answer
  • one involves hydrogen bonding while the other does not
  • one involves dipole attraction between neutral molecules while the other involves dipole interactions with ions
  • one involves salts and water while the other doesn't involve water
  • one involves ionic molecules interacting with other ionic molecules while the other deals with polar molecules
  • none of the above

Question 9

Question
How is it possible for a neutral molecule, such as water, to form an ion?
Answer
  • It can fragment into protons and electrons.
  • It can combine with a chloride ion to form a negatively charged species.
  • It can absorb electrons and become negatively charged.
  • It can combine with a hydrogen ion to form a positively charged species.
  • It can absorb electrons and become positively charged.

Question 10

Question
How do the electron-dot structures of elements in the same group in the periodic table compare with one another?
Answer
  • The number of electrons in the electron-dot-structure will equal the group number for each element of the group.
  • The structures differ by exactly two electrons between vertically consecutive elements.
  • Elements of the same group have the same number of valence electrons.
  • The number of valence shell electrons increases by one for each element from the top to the bottom of the group.

Question 11

Question
Which of the following elements will most likely form an ion with a -2 charge?
Answer
  • Mg
  • S
  • Cl
  • Ne
  • Na

Question 12

Question
Many of the macroscopic properties of a compound depend on ________.
Answer
  • the mass of the constituent atoms
  • how the atoms of the molecules are held together
  • the number of nucleons present in the sample
  • the size of the sample
  • how the atoms absorb light and the shape of the orbitals

Question 13

Question
Which of the following statements describes a polar molecule?
Answer
  • The molecules are usually not attracted to one another very strongly.
  • Polar molecules have the weakest intermolecular interactions with ionic compounds.
  • The electrons in the molecule are distributed evenly throughout the molecule.
  • The molecules have a high degree of symmetry.
  • None of these statements describe polar molecules.

Question 14

Question
Metals are useful for the structural support of buildings because they
Answer
  • do not conduct heat well
  • are strong but can be bent
  • conduct electricity
  • are shiny
  • c and d

Question 15

Question
Which of the following statements best describes a relatively polar bond?
Answer
  • a very electronegative atom and a weakly electronegative atom are covalently bound
  • two very electronegative atoms undergo ionic bonding
  • two very electronegative atoms are covalently bound
  • two weakly electronegative atoms undergo ionic bonding
  • none of the above

Question 16

Question
What property of metal atoms account for many of the observed bulk phenomena seen in metal samples?
Answer
  • Metals readily form covalent bonds.
  • Metal atoms easily lose one or more outer electrons.
  • Metals readily form ionic bonds.
  • Metal atoms easily gain one or more outer electrons.
  • none of the above

Question 17

Question
Which of the following is NOT an ion?
Answer
  • Mg+2
  • NO3-
  • H+1
  • O2
  • Br-

Question 18

Question
If a neutral atom loses one electron, what is the electrical charge of the atom?
Answer
  • +2
  • -2
  • +1
  • -1
  • neutral

Question 19

Question
How many more electrons can fit within the valence shell of a hydrogen atom?
Answer
  • 7
  • 2
  • 0
  • 1

Question 20

Question
What is the main difference between a dipole-dipole interaction and a dipole-induced dipole interaction?
Answer
  • Dipole-induced dipole interactions are stronger because the induced dipoles can be formed at any time.
  • Dipole-dipole interactions are weaker because the dipoles are permanent.
  • Both are similar, but one involves a temporary dipole created by a permanent dipole.
  • Both are identical.
  • none of the above

Question 21

Question
Distinguish between a metal and a metal-containing compound.
Answer
  • Only one of these contains ionic bonds.
  • Only one of these contains covalent bonds.
  • There is no distinction between the two.
  • Only one of these occurs naturally.

Question 22

Question
Which of the following describes how a metal atoms behaves in a bulk metallic object?
Answer
  • The metal atoms have limited interaction with neighboring atoms.
  • The metal atom shares its electrons in a very directional manner.
  • The metal atom shares its electrons with only one other atom.
  • The metal ion shares its outermost electrons freely with its neighbors.
  • none of the above

Question 23

Question
How is the number of unpaired valence electrons in an atom related to the number of bonds that the atom can form?
Answer
  • There is no defined relationship between the number of unpaired valence electrons and number of bonds that the atom can form.
  • The number of unpaired valence electrons in an atom is the same as the number of bonds that the atom can form.
  • The number of unpaired valence electrons in an atom is twice the number of bonds that the atom can form.
  • The number of unpaired valence electrons in an atom is one-half the number of bonds that the atom can form.

Question 24

Question
Which of the following does not describe ionic compounds?
Answer
  • They have a tendency to melt easily.
  • They are usually very ordered.
  • They consist of positive and negative ions.
  • They are held together by electrostatic attraction.
  • none of the above

Question 25

Question
Atoms of nonmetallic elements form covalent bonds, but they can also form ionic bonds. How is this possible?
Answer
  • An ionic bond results when a nonmetallic elements gains an electron from a metallic element.
  • This happens when one of the bonded nonmetallic elements has a strong electronegativity.
  • It happens when one of the nonmetallic elements loses an electron to become a positive ion.
  • An ionic bond results when a nonmetallic elements loses an electron to a metallic element.

Question 26

Question
In a solution of 77 percent nitrogen and 23 percent oxygen, which is the solvent?
Answer
  • nitrogen
  • oxygen
  • both
  • neither
  • gases cannot form solutions

Question 27

Question
If you filter sea water to remove all of the particles you would be left with a clear ________.
Answer
  • homogeneous mixture called a suspension
  • heterogeneous mixture called a solution
  • heterogeneous mixture called a suspension
  • pure liquid
  • homogeneous mixture called a solution

Question 28

Question
How would you classify the following material? milk
Answer
  • a solution
  • a compound
  • a suspension
  • an element
  • a heterogeneous mixture

Question 29

Question
The following image represents which kind of matter?
Answer
  • a compound
  • an element
  • a mixture
  • none of the above
  • all of the above

Question 30

Question
Which of the following accurately describes osmosis?
Answer
  • The less concentrated solution gets more dilute.
  • The more concentrated solution absorbs water from the less concentrated solution.
  • The less concentrated solution absorbs water from the more concentrated solution.
  • The ions migrate from the more concentrated solution to the less concentrated.
  • none of the above

Question 31

Question
What is the difference between a compound and a mixture?
Answer
  • The components of a mixture do not have the same properties individually as they do when mixed.
  • A compound can be physically separated into its components; a mixture cannot be physically separated into its components.
  • A compound is just a mixture of elements.
  • A mixture can be physically separated into its components; a compound cannot be physically separated into its components.
  • The components of a compound have the same properties individually as they do when mixed.

Question 32

Question
A combination of two or more substances in which they no longer retain their chemical properties is called a(n) ________.
Answer
  • compound
  • heterogeneous mixture
  • periodic trend
  • suspension
  • mixture

Question 33

Question
What is the difference between a compound and a mixture?
Answer
  • The components of a mixture are not chemically bonded together.
  • They both consist of atoms from different elements.
  • The way in which their atoms are bonded together.
  • One is a solid and the other is a liquid.

Question 34

Question
Which of the following solutions is the most concentrated?
Answer
  • one liter of water with 5 grams of sugar
  • one liter of water with 10 grams of sugar
  • one liter of water with 1 gram of sugar
  • one liter of water with 2 grams of sugar
  • They all have the same volume

Question 35

Question
What is the purpose of treating water with chlorine gas or ozone during water purification?
Answer
  • to improve taste
  • to kill bacteria
  • to improve color
  • to remove solids
  • none of the above

Question 36

Question
How would you classify the following material? coffee (black)
Answer
  • an element
  • a solution
  • a heterogeneous mixture
  • a compound
  • a suspension

Question 37

Question
In a solution made from one teaspoon of sugar and one liter of water, which is the solute?
Answer
  • sugar
  • the teaspoon
  • water
  • both sugar and water
  • none of the above

Question 38

Question
Mixtures can be separated into their components by taking advantage of differences in the chemical properties of the components. Why might this separation method be less convenient than taking advantage of differences in the physical properties of the components?
Answer
  • The chemical properties of the components of a mixture are too different from each other.
  • The chemical properties of the components of a mixture are too similar to each other.
  • A chemical property involves a chemical change so that you no longer have what you had.
  • Chemical properties are not as apparent as are physical properties.

Question 39

Question
How would you classify the following material? coffee (with milk)
Answer
  • an element
  • a compound
  • a suspension
  • a heterogeneous mixture
  • a solution

Question 40

Question
Which of the following is not a typical use for potable water?
Answer
  • cooking in a pot
  • flushing a toilet
  • boiling
  • irrigation
  • drinking

Question 41

Question
Which has the most atoms?
Answer
  • a mole of helium
  • a mole of gold
  • a mole of lead
  • All of the above have the same number of atoms.
  • none of the above

Question 42

Question
When blue food coloring is stirred into water, the result is a ________.
Answer
  • homogeneous mixture called a suspension
  • heterogeneous mixture called a suspension
  • heterogeneous mixture called a solution
  • pure liquid
  • homogeneous mixture called a solution

Question 43

Question
Which of the following solutions is the most concentrated?
Answer
  • 0.1 liter of water with 1 gram of sugar
  • 0.5 liter of water with 50 grams of sugar
  • 2 liters of water with 0.2 gram of sugar
  • 3 liters of water with 30 grams of sugar
  • They all have the same concentration.

Question 44

Question
How might you separate a mixture of sand and salt?
Answer
  • just add water
  • with tweezers and a magnifying glass
  • heat the mixture until one of the components melts
  • Two of the above answers are reasonable.

Question 45

Question
How would you classify the following material? a cappuccino (with foam)
Answer
  • a solution
  • a heterogeneous mixture
  • a suspension
  • a compound
  • an element

Question 46

Question
Why can't the elements of a compound be separated from one another by physical means?
Answer
  • Elements found within a compound tend to be inert.
  • They are too homogeneous when found within a compound.
  • Elements tend not to be soluble in water.
  • Their atoms are too tightly bound to one another.

Question 47

Question
Why is secondary treatment often needed for sewage?
Answer
  • The solution is contaminated with dangerous bacteria.
  • The dissolved organics are too high and lead to bacterial growth.
  • There are too many finely divided particles that need to be filtered.
  • There are too many dissolved inorganic compounds.
  • none of the above

Question 48

Question
What do chicken noodle soup and garden soil have in common?
Answer
  • They are both examples of compounds.
  • They both contain elements.
  • They are both examples of heterogeneous mixtures.
  • nothing

Question 49

Question
Which of the following statements about sewage is not true?
Answer
  • Treated sewage becomes drinking water downstream.
  • All municipalities must treat sewage the same way.
  • All municipalities must treat sewage.
  • Once treated, sewage is released to the environment.
  • None of the above are true.

Question 50

Question
How is the solubility of a solid affected by temperature?
Answer
  • As temperature goes up, the solubility goes up.
  • As temperature goes down, the solubility goes down.
  • As temperature goes down, the solubility goes up.
  • As temperature goes up, the solubility goes down.
  • both A and B : (As temperature goes up, the solubility goes up. As temperature goes down, the solubility goes down.)

Question 51

Question
Which of the following elements has six valence electrons?
Answer
  • Be
  • B
  • N
  • C
  • O

Question 52

Question
Which of the following molecules contains a polar bond?
Answer
  • F-F
  • Cl-Cl
  • H-H
  • H-F
  • all of the above

Question 53

Question
If you mix a typical aluminum ion (Al, atomic no. = 13) with a typical oxygen ion (O, atomic no. = 8), what compound is formed?
Answer
  • Al2O3
  • Al13O8
  • Al3O2
  • Al3O
  • Al2O2

Question 54

Question
How many valence electrons does gallium (Ga, atomic no. = 31) have?
Answer
  • 1
  • 31
  • 3
  • 6
  • 70

Question 55

Question
Which of the following elements will most likely form an ion with a -1 charge?
Answer
  • Ne
  • Cl
  • S
  • Na
  • Mg

Question 56

Question
Which of the following compounds has polar covalent bonds?
Answer
  • CsF2
  • S8
  • CH4
  • H2O
  • Ne

Question 57

Question
What it the main difference between an ionic and a covalent bond?
Answer
  • One involves electrons, the other does not involve any electrons.
  • Both bonds are the same, but named different to describe different atoms involved.
  • One is the sharing of a pair of electrons, the other is the transfer of at least one electron.
  • The electrons are traded between the two atoms and this keeps the atoms close.

Question 58

Question
If you mix a typical iodine ion (I, atomic no. = 53) with a typical barium ion (Ba, atomic no. = 56), what compound is formed?
Answer
  • BaI
  • Ba56I53
  • Ba2I2
  • BaI2
  • Ba2I

Question 59

Question
Barium ions carry a 2+ charge, and nitrogen ions carry a 3-charge. What would be the chemical formula for the ionic compound barium nitride?
Answer
  • Ba3N4
  • Ba3N2
  • Ba2N2
  • Ba2N3

Question 60

Question
What does the line in the following example actually represent? H—H
Answer
  • a shared pair of electrons
  • a covalent bond
  • an ionic bond
  • a pair of nonbonding electrons
  • A and B: a shared pair of electrons, a covalent bond

Question 61

Question
Does an ionic bond have a dipole?
Answer
  • No, dipoles are only found in covalent compounds.
  • Yes, the ionic bond is an example of a very strong dipole.
  • No, but the electrical charges are relatively strong.
  • Yes, but for ionic compounds they are referred to as monopoles.

Question 62

Question
The concept of a chemical bond is ________.
Answer
  • how two or more electrons reside in an orbital
  • the sharing of nucleons
  • how two or more atoms are held together
  • how much energy it takes to remove an electron from a set of atoms
  • none of the above

Question 63

Question
What is one role of unpaired valance electrons?
Answer
  • They are the nonbonding electrons.
  • They tell us which Lewis dot structure is correct.
  • They take part in the formation of different types of bonds.
  • They keep the paired electrons separated to minimize interaction.
  • They provide the number of Lewis dots.

Question 64

Question
What is a molecule?
Answer
  • group of covalent compounds held together by ionic bonds
  • pair of shared valence electrons
  • a group of atoms that are held together by ionic bonds
  • a group of atoms that are held together by covalent bonds
  • pair of atoms sharing a set of valence electron

Question 65

Question
In terms of the periodic table, is there an abrupt or gradual change between ionic and covalent bonds?
Answer
  • There is a gradual change: the farther apart, the more ionic.
  • There is an abrupt change that occurs across the metalloids
  • Whether an element forms one or the other depends on nuclear charge and not the relative positions in the periodic table.
  • Actually, any element of the periodic table can form a covalent bond.

Question 66

Question
What is the difference between a dipole-dipole interaction and an ion-dipole interaction?
Answer
  • one involves hydrogen bonding while the other does not
  • one involves dipole attraction between neutral molecules while the other involves dipole interactions with ions
  • one involves salts and water while the other doesn't involve water
  • one involves ionic molecules interacting with other ionic molecules while the other deals with polar molecules
  • none of the above

Question 67

Question
How is the solubility of a solid affected by temperature?
Answer
  • As temperature goes up, the solubility goes up.
  • As temperature goes down, the solubility goes down.
  • As temperature goes down, the solubility goes up.
  • As temperature goes up, the solubility goes down.
  • both A and B (As temperature goes up, the solubility goes up. As temperature goes down, the solubility goes down.)

Question 68

Question
What is the first step in treating raw sewage?
Answer
  • removal of sludge
  • removal of grit by settling
  • filtration of solids
  • disinfection
  • removal of fine particles by settling

Question 69

Question
What statement best describes a mole?
Answer
  • It is a very large number chemists use to count atoms or molecules.
  • the amount of molecules or atoms in 1 gram of something
  • a very small number chemists use to count atoms or molecules
  • a little furry mammal that lives in the ground
  • none of the above

Question 70

Question
Which of the following would be considered a homogeneous mixture?
Answer
  • hydrogen cyanide
  • wine
  • pretzel
  • rusty iron
  • sugar

Question 71

Question
Which of the following solutions is the most dilute?
Answer
  • one liter of water with 10 grams of sugar
  • one liter of water with 5 grams of sugar
  • one liter of water with 2 grams of sugar
  • one liter of water with 1 gram of sugar
  • They all have the same volume.

Question 72

Question
Which of the following is a pure substance?
Answer
  • salt water
  • orange juice
  • baking soda
  • duct tape
  • cooking oil

Question 73

Question
The following image represents which kind of matter?
Answer
  • a compound
  • an element
  • a mixture
  • none of the above
  • all of the above

Question 74

Question
A sample of steel is composed of 5 percent carbon and 95 percent iron. Which is the solvent?
Answer
  • carbon
  • iron
  • steel
  • Steel is not a solution, it is a mixture.
  • A solid cannot be a solvent.

Question 75

Question
Which of the following material phases cannot form a solution?
Answer
  • solids
  • gases
  • liquids
  • All of the above can form solutions.
  • None of the above can form solutions.

Question 76

Question
How does a suspension differ from a solution?
Answer
  • A suspension is a heterogeneous mixture consisting of different phases whereas a solution is a homogeneous mixture consisting of a single phase.
  • The difference between a suspension and a solution can only be determined by chemical means.
  • A suspension is a heterogeneous mixture whose components can be separated by simple filtration. A solution is a homogeneous mixture which cannot be separated by simple filtration.
  • Although a solution and suspension are both homogeneous mixtures, only the components of a suspension will separate by spinning the mixture in a centrifuge.

Question 77

Question
How would you classify the following material? swimming pool water
Answer
  • heterogeneous mixture
  • a pure element
  • a pure compound
  • homogeneous mixture
  • depends on how many children have been in it

Question 78

Question
Which of the following bonds would be the most polar?
Answer
  • C-Cl
  • C-Br
  • C-F
  • C-I
  • All are equally polar.

Question 79

Question
Which of the following bonds would be the least polar?
Answer
  • C-H
  • C-F
  • C-O
  • C-Cl
  • All are equally polar.

Question 80

Question
Which of the following elements will most likely not form an ion at all?
Answer
  • Na
  • Mg
  • Br
  • O
  • Ar

Question 81

Question
Which of the following is the weakest?
Answer
  • A dipole-induced dipole attraction
  • A dipole-dipole attraction
  • An induced dipole-induced dipole attraction
  • An ion-dipole attraction
  • A chemical bond

Question 82

Question
Which of the following compounds contains ionic bonds?
Answer
  • CH4
  • OF2
  • Cl2
  • K2O
  • none of the above

Question 83

Question
Which of the following molecules is the most polar?
Answer
  • HCl
  • BrF
  • Br2
  • CO

Question 84

Question
Which of the following statements is untrue?
Answer
  • Covalent molecules usually have low melting points.
  • Covalent molecules can have nonbonding electrons.
  • Covalent bonds can involve more than one pair of electrons.
  • Covalent molecules are never crystalline.
  • All of the above statements are true.

Question 85

Question
Which of the following elements will most likely form an ion with a +1 charge?
Answer
  • Al
  • Mg
  • Cl
  • Na
  • Si

Question 86

Question
Which of the following is not a property of metal?
Answer
  • conducts electricity
  • is strong, but can be bent
  • does not conduct heat well
  • is shiny
  • All of the above are properties of metals.

Question 87

Question
Is an ionic compound an example of a chemical compound, or is a chemical compound an example of an ionic compound?
Answer
  • An ionic compound is an example of a chemical compound.
  • Each is an example of the other.
  • An chemical compound is an example of a ionic compound.
  • Neither is an example of the other.

Question 88

Question
Which of the following statements describes a saturated solution?
Answer
  • a solution of salt water with salt at the bottom
  • a carbonated beverage with bubbles
  • a solution where the solvent cannot dissolve any more solute
  • all of the above
  • none of the above

Question 89

Question
What is molarity?
Answer
  • the number of liters of solute per mole of solution
  • the number of moles of solute per liter of solution
  • the number of moles of solute per liter of solvent
  • the number of grams of solute per liter of solution
  • none of the above

Question 90

Question
The following image represents which kind of matter?
Answer
  • an element
  • a mixture
  • a compound
  • none of the above
  • all of the above

Question 91

Question
Is the air in your house a homogeneous or heterogeneous mixture?
Answer
  • heterogeneous because of the dust particles it contains
  • homogeneous because it is all at the same temperature
  • homogeneous because it is mixed very well
  • heterogeneous because it consists of different types of molecules

Question 92

Question
Which of the following would be considered a heterogeneous mixture?
Answer
  • water
  • milk
  • vinegar
  • vegetable oil
  • salad dressing

Question 93

Question
Which of the following is a mixture?
Answer
  • helium
  • iron
  • air
  • gold
  • salt

Question 94

Question
How is the solubility of a gas affected by temperature?
Answer
  • As temperature goes up, the solubility goes up
  • As temperature goes up, the solubility stays the same.
  • As temperature goes down, the solubility goes down.
  • As temperature goes down, the solubility goes up.
  • both A and B
Show full summary Hide full summary

Want to create your own Quizzes for free with GoConqr? Learn more.

Similar

Plate Tectonics
Selam H
ANZCA Part 2 MCQs - 2015
Branden Emmerson
Exam 3
Kimberly Lopez
MCAT Study Plan
Alice McClean
AP Chemistry
Cathal Darby
Microbiology MCQs 3rd Year Final- PMU
Med Student
Anatomy and Physiology
pressey_property
Science Final Study Guide
Caroline Conlan
APUSH End-of-Year Cram Exam: Set 1
Nathaniel Rodriguez
sec + final
maxwell3254
CCNA Security Final Exam
Maikel Degrande
Browse Library