Kimberly Lopez
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Conceptual physical science

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Kimberly Lopez
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Exam 2

Question 1 of 94

1

What is the valence shell?

Select one of the following:

  • 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.

Explanation

Question 2 of 94

1

Which of the following best describes ionic bonding?

Select one of the following:

  • 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

Explanation

Question 3 of 94

1

How many valence electrons does bromine (Br, atomic no. = 35) have?

Select one of the following:

  • 28

  • 7

  • 21

  • 1

  • 35

Explanation

Question 4 of 94

1

The source of an atom's electronegativity is the

Select one of the following:

  • 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.

Explanation

Question 5 of 94

1

Metals are often used for making designer jewelry because they

Select one of the following:

  • 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)

Explanation

Question 6 of 94

1

Which of the following is the main form of intermolecular attractions among water molecules?

Select one of the following:

  • hydrogen bonding

  • induced dipole-induced dipole

  • polar-induced polar

  • ion-dipole

  • covalent bonding

Explanation

Question 7 of 94

1

If a neutral atom gains two electrons, what is the electrical charge of the atom?

Select one of the following:

  • +1

  • +2

  • neutral

  • -1

  • -2

Explanation

Question 8 of 94

1

What is the difference between a dipole-dipole interaction and an ion-dipole interaction?

Select one of the following:

  • 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

Explanation

Question 9 of 94

1

How is it possible for a neutral molecule, such as water, to form an ion?

Select one of the following:

  • 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.

Explanation

Question 10 of 94

1

How do the electron-dot structures of elements in the same group in the periodic table compare with one another?

Select one of the following:

  • 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.

Explanation

Question 11 of 94

1

Which of the following elements will most likely form an ion with a -2 charge?

Select one of the following:

  • Mg

  • S

  • Cl

  • Ne

  • Na

Explanation

Question 12 of 94

1

Many of the macroscopic properties of a compound depend on ________.

Select one of the following:

  • 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

Explanation

Question 13 of 94

1

Which of the following statements describes a polar molecule?

Select one of the following:

  • 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.

Explanation

Question 14 of 94

1

Metals are useful for the structural support of buildings because they

Select one of the following:

  • do not conduct heat well

  • are strong but can be bent

  • conduct electricity

  • are shiny

  • c and d

Explanation

Question 15 of 94

1

Which of the following statements best describes a relatively polar bond?

Select one of the following:

  • 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

Explanation

Question 16 of 94

1

What property of metal atoms account for many of the observed bulk phenomena seen in metal samples?

Select one of the following:

  • 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

Explanation

Question 17 of 94

1

Which of the following is NOT an ion?

Select one of the following:

  • Mg+2

  • NO3-

  • H+1

  • O2

  • Br-

Explanation

Question 18 of 94

1

If a neutral atom loses one electron, what is the electrical charge of the atom?

Select one of the following:

  • +2

  • -2

  • +1

  • -1

  • neutral

Explanation

Question 19 of 94

1

How many more electrons can fit within the valence shell of a hydrogen atom?

Select one of the following:

  • 7

  • 2

  • 0

  • 1

Explanation

Question 20 of 94

1

What is the main difference between a dipole-dipole interaction and a dipole-induced dipole interaction?

Select one of the following:

  • 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

Explanation

Question 21 of 94

1

Distinguish between a metal and a metal-containing compound.

Select one of the following:

  • 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.

Explanation

Question 22 of 94

1

Which of the following describes how a metal atoms behaves in a bulk metallic object?

Select one of the following:

  • 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

Explanation

Question 23 of 94

1

How is the number of unpaired valence electrons in an atom related to the number of bonds that the atom can form?

Select one of the following:

  • 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.

Explanation

Question 24 of 94

1

Which of the following does not describe ionic compounds?

Select one of the following:

  • 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

Explanation

Question 25 of 94

1

Atoms of nonmetallic elements form covalent bonds, but they can also form ionic bonds. How is this possible?

Select one of the following:

  • 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.

Explanation

Question 26 of 94

1

In a solution of 77 percent nitrogen and 23 percent oxygen, which is the solvent?

Select one of the following:

  • nitrogen

  • oxygen

  • both

  • neither

  • gases cannot form solutions

Explanation

Question 27 of 94

1

If you filter sea water to remove all of the particles you would be left with a clear ________.

Select one of the following:

  • homogeneous mixture called a suspension

  • heterogeneous mixture called a solution

  • heterogeneous mixture called a suspension

  • pure liquid

  • homogeneous mixture called a solution

Explanation

Question 28 of 94

1

How would you classify the following material?

milk

Select one of the following:

  • a solution

  • a compound

  • a suspension

  • an element

  • a heterogeneous mixture

Explanation

Question 29 of 94

1

The following image represents which kind of matter?

Select one of the following:

  • a compound

  • an element

  • a mixture

  • none of the above

  • all of the above

Explanation

Question 30 of 94

1

Which of the following accurately describes osmosis?

Select one of the following:

  • 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

Explanation

Question 31 of 94

1

What is the difference between a compound and a mixture?

Select one of the following:

  • 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.

Explanation

Question 32 of 94

1

A combination of two or more substances in which they no longer retain their chemical properties is called a(n) ________.

Select one of the following:

  • compound

  • heterogeneous mixture

  • periodic trend

  • suspension

  • mixture

Explanation

Question 33 of 94

1

What is the difference between a compound and a mixture?

Select one of the following:

  • 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.

Explanation

Question 34 of 94

1

Which of the following solutions is the most concentrated?

Select one of the following:

  • 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

Explanation

Question 35 of 94

1

What is the purpose of treating water with chlorine gas or ozone during water purification?

Select one of the following:

  • to improve taste

  • to kill bacteria

  • to improve color

  • to remove solids

  • none of the above

Explanation

Question 36 of 94

1

How would you classify the following material?

coffee (black)

Select one of the following:

  • an element

  • a solution

  • a heterogeneous mixture

  • a compound

  • a suspension

Explanation

Question 37 of 94

1

In a solution made from one teaspoon of sugar and one liter of water, which is the solute?

Select one of the following:

  • sugar

  • the teaspoon

  • water

  • both sugar and water

  • none of the above

Explanation

Question 38 of 94

1

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?

Select one of the following:

  • 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.

Explanation

Question 39 of 94

1

How would you classify the following material?

coffee (with milk)

Select one of the following:

  • an element

  • a compound

  • a suspension

  • a heterogeneous mixture

  • a solution

Explanation

Question 40 of 94

1

Which of the following is not a typical use for potable water?

Select one of the following:

  • cooking in a pot

  • flushing a toilet

  • boiling

  • irrigation

  • drinking

Explanation

Question 41 of 94

1

Which has the most atoms?

Select one of the following:

  • 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

Explanation

Question 42 of 94

1

When blue food coloring is stirred into water, the result is a ________.

Select one of the following:

  • homogeneous mixture called a suspension

  • heterogeneous mixture called a suspension

  • heterogeneous mixture called a solution

  • pure liquid

  • homogeneous mixture called a solution

Explanation

Question 43 of 94

1

Which of the following solutions is the most concentrated?

Select one of the following:

  • 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.

Explanation

Question 44 of 94

1

How might you separate a mixture of sand and salt?

Select one of the following:

  • 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.

Explanation

Question 45 of 94

1

How would you classify the following material?

a cappuccino (with foam)

Select one of the following:

  • a solution

  • a heterogeneous mixture

  • a suspension

  • a compound

  • an element

Explanation

Question 46 of 94

1

Why can't the elements of a compound be separated from one another by physical means?

Select one of the following:

  • 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.

Explanation

Question 47 of 94

1

Why is secondary treatment often needed for sewage?

Select one of the following:

  • 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

Explanation

Question 48 of 94

1

What do chicken noodle soup and garden soil have in common?

Select one of the following:

  • They are both examples of compounds.

  • They both contain elements.

  • They are both examples of heterogeneous mixtures.

  • nothing

Explanation

Question 49 of 94

1

Which of the following statements about sewage is not true?

Select one of the following:

  • 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.

Explanation

Question 50 of 94

1

How is the solubility of a solid affected by temperature?

Select one of the following:

  • 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.)

Explanation

Question 51 of 94

1

Which of the following elements has six valence electrons?

Select one of the following:

  • Be

  • B

  • N

  • C

  • O

Explanation

Question 52 of 94

1

Which of the following molecules contains a polar bond?

Select one of the following:

  • F-F

  • Cl-Cl

  • H-H

  • H-F

  • all of the above

Explanation

Question 53 of 94

1

If you mix a typical aluminum ion (Al, atomic no. = 13) with a typical oxygen ion (O, atomic no. = 8), what compound is formed?

Select one of the following:

  • Al2O3

  • Al13O8

  • Al3O2

  • Al3O

  • Al2O2

Explanation

Question 54 of 94

1

How many valence electrons does gallium (Ga, atomic no. = 31) have?

Select one of the following:

  • 1

  • 31

  • 3

  • 6

  • 70

Explanation

Question 55 of 94

1

Which of the following elements will most likely form an ion with a -1 charge?

Select one of the following:

  • Ne

  • Cl

  • S

  • Na

  • Mg

Explanation

Question 56 of 94

1

Which of the following compounds has polar covalent bonds?

Select one of the following:

  • CsF2

  • S8

  • CH4

  • H2O

  • Ne

Explanation

Question 57 of 94

1

What it the main difference between an ionic and a covalent bond?

Select one of the following:

  • 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.

Explanation

Question 58 of 94

1

If you mix a typical iodine ion (I, atomic no. = 53) with a typical barium ion (Ba, atomic no. = 56), what compound is formed?

Select one of the following:

  • BaI

  • Ba56I53

  • Ba2I2

  • BaI2

  • Ba2I

Explanation

Question 59 of 94

1

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?

Select one of the following:

  • Ba3N4

  • Ba3N2

  • Ba2N2

  • Ba2N3

Explanation

Question 60 of 94

1

What does the line in the following example actually represent?

H—H

Select one of the following:

  • 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

Explanation

Question 61 of 94

1

Does an ionic bond have a dipole?

Select one of the following:

  • 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.

Explanation

Question 62 of 94

1

The concept of a chemical bond is ________.

Select one of the following:

  • 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

Explanation

Question 63 of 94

1

What is one role of unpaired valance electrons?

Select one of the following:

  • 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.

Explanation

Question 64 of 94

1

What is a molecule?

Select one of the following:

  • 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

Explanation

Question 65 of 94

1

In terms of the periodic table, is there an abrupt or gradual change between ionic and covalent bonds?

Select one of the following:

  • 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.

Explanation

Question 66 of 94

1

What is the difference between a dipole-dipole interaction and an ion-dipole interaction?

Select one of the following:

  • 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

Explanation

Question 67 of 94

1

How is the solubility of a solid affected by temperature?

Select one of the following:

  • 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.)

Explanation

Question 68 of 94

1

What is the first step in treating raw sewage?

Select one of the following:

  • removal of sludge

  • removal of grit by settling

  • filtration of solids

  • disinfection

  • removal of fine particles by settling

Explanation

Question 69 of 94

1

What statement best describes a mole?

Select one of the following:

  • 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

Explanation

Question 70 of 94

1

Which of the following would be considered a homogeneous mixture?

Select one of the following:

  • hydrogen cyanide

  • wine

  • pretzel

  • rusty iron

  • sugar

Explanation

Question 71 of 94

1

Which of the following solutions is the most dilute?

Select one of the following:

  • 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.

Explanation

Question 72 of 94

1

Which of the following is a pure substance?

Select one of the following:

  • salt water

  • orange juice

  • baking soda

  • duct tape

  • cooking oil

Explanation

Question 73 of 94

1

The following image represents which kind of matter?

Select one of the following:

  • a compound

  • an element

  • a mixture

  • none of the above

  • all of the above

Explanation

Question 74 of 94

1

A sample of steel is composed of 5 percent carbon and 95 percent iron. Which is the solvent?

Select one of the following:

  • carbon

  • iron

  • steel

  • Steel is not a solution, it is a mixture.

  • A solid cannot be a solvent.

Explanation

Question 75 of 94

1

Which of the following material phases cannot form a solution?

Select one of the following:

  • solids

  • gases

  • liquids

  • All of the above can form solutions.

  • None of the above can form solutions.

Explanation

Question 76 of 94

1

How does a suspension differ from a solution?

Select one of the following:

  • 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.

Explanation

Question 77 of 94

1

How would you classify the following material?

swimming pool water

Select one of the following:

  • heterogeneous mixture

  • a pure element

  • a pure compound

  • homogeneous mixture

  • depends on how many children have been in it

Explanation

Question 78 of 94

1

Which of the following bonds would be the most polar?

Select one of the following:

  • C-Cl

  • C-Br

  • C-F

  • C-I

  • All are equally polar.

Explanation

Question 79 of 94

1

Which of the following bonds would be the least polar?

Select one of the following:

  • C-H

  • C-F

  • C-O

  • C-Cl

  • All are equally polar.

Explanation

Question 80 of 94

1

Which of the following elements will most likely not form an ion at all?

Select one of the following:

  • Na

  • Mg

  • Br

  • O

  • Ar

Explanation

Question 81 of 94

1

Which of the following is the weakest?

Select one of the following:

  • A dipole-induced dipole attraction

  • A dipole-dipole attraction

  • An induced dipole-induced dipole attraction

  • An ion-dipole attraction

  • A chemical bond

Explanation

Question 82 of 94

1

Which of the following compounds contains ionic bonds?

Select one of the following:

  • CH4

  • OF2

  • Cl2

  • K2O

  • none of the above

Explanation

Question 83 of 94

1

Which of the following molecules is the most polar?

Select one of the following:

  • HCl

  • BrF

  • Br2

  • CO

Explanation

Question 84 of 94

1

Which of the following statements is untrue?

Select one of the following:

  • 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.

Explanation

Question 85 of 94

1

Which of the following elements will most likely form an ion with a +1 charge?

Select one of the following:

  • Al

  • Mg

  • Cl

  • Na

  • Si

Explanation

Question 86 of 94

1

Which of the following is not a property of metal?

Select one of the following:

  • conducts electricity

  • is strong, but can be bent

  • does not conduct heat well

  • is shiny

  • All of the above are properties of metals.

Explanation

Question 87 of 94

1

Is an ionic compound an example of a chemical compound, or is a chemical compound an example of an ionic compound?

Select one of the following:

  • 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.

Explanation

Question 88 of 94

1

Which of the following statements describes a saturated solution?

Select one of the following:

  • 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

Explanation

Question 89 of 94

1

What is molarity?

Select one of the following:

  • 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

Explanation

Question 90 of 94

1

The following image represents which kind of matter?

Select one of the following:

  • an element

  • a mixture

  • a compound

  • none of the above

  • all of the above

Explanation

Question 91 of 94

1

Is the air in your house a homogeneous or heterogeneous mixture?

Select one of the following:

  • 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

Explanation

Question 92 of 94

1

Which of the following would be considered a heterogeneous mixture?

Select one of the following:

  • water

  • milk

  • vinegar

  • vegetable oil

  • salad dressing

Explanation

Question 93 of 94

1

Which of the following is a mixture?

Select one of the following:

  • helium

  • iron

  • air

  • gold

  • salt

Explanation

Question 94 of 94

1

How is the solubility of a gas affected by temperature?

Select one of the following:

  • 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

Explanation

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