Chemistry

Question 1

What branch of chemistry studies
carbon compounds such as fuels, food
additives and drugs?

A. Organic chemistry
B. Inorganic chemistry
C. Biochemistry
D. Analytical chemistry

Answer 1

A. Organic chemistry

Organic Chemistry - branch of
chemistry deals with the chemistry of
carbon and living things.

Inorganic Chemistry - branch of
chemistry that deals with the structure
and interactions between inorganic
compounds, which are any compounds that are not based in carbon-hydrogen bonds.

Biochemistry - branch of chemistry
concerned with the chemical reactions
that occur inside living organisms.

Analytical Chemistry - branch of
chemistry involved with studying the properties of materials or developing tools to analyze materials.

Question 2

Which of the following is an intensive
property?

A. Mass
B. Density
C. Volume
D. Number of atoms

Answer 2

B. Density

Intensive Properties - are properties that are independent on the size of the sample involved.
Examples: density, freezing point, color,
melting point, reactivity, luster,
malleability, conductivity, etc.

Question 3

The process in which a gas changes
directly into its solid without first
forming a liquid is called _____

A. Sublimation
B. Deposition
C. Calcination
D. Isolation

Answer 3

B. Deposition

(CHEM FIGURE)

Question 4

Which of the following is an extensive
property of a bubble of air?

A. Temperature
B. Density
C. Percent oxygen
D. Radius

Answer 4

D. Radius

Extensive Properties - are properties that depend on the size of the sample involved.
Examples: volume, mass, weight, length,
etc.

Question 5

Which of the following is an intensive
chemical property of a box of raisins?

A. grams per serving
B. total number of raisins
C. total calories
D. calories per serving

Answer 5

D. calories per serving

Chemical Properties - are properties that lead to changes in the identity and composition of a substance.
Examples: combustibility, pH, tendency
to rust, reaction with water, etc.
Intensive Properties - are properties that are independent on the size of the sample involved.
Examples: density, freezing point, color,
melting point, reactivity, luster,
malleability, conductivity, etc.

Question 6

Which of the following is an extensive
property?

A. Color
B. Temperature
C. Melting point
D. Volume

Answer 6

D. Volume

Extensive Properties - are properties that depend on the size of the sample involved.
Examples: volume, mass, weight, length,
etc.

Question 7

The specific volume of a substance is
the volume per gram of substance.
Specific volume is an example of

A. a physical, intensive property
B. a chemical, extensive property
C. a chemical, intensive property
D. a physical, extensive property

Answer 7

A. a physical, intensive property

Physical Properties - are properties
which can be measured without
changing the identity and composition
of a substance.
Examples: odor, color, density, boiling point, melting point, polarity,solubility,opacity, viscosity, etc.
Intensive Properties - are properties that are independent on the size of the sample involved.
Examples: density, freezing point, color,
melting point, reactivity, luster,
malleability, conductivity, etc.

Question 8

Which of the following is an extensive
property of coffee in a mug?

A. temperature
B. total mg of caffeine
C. cream added per mL of coffee
D. percent sugar

Answer 8

B. total mg of caffeine

Extensive Properties - are properties that depend on the size of the sample involved.
Examples: volume, mass, weight, length,
etc.

Question 9

Which of the following is a physical
property?

A. Temperature
B. Corrosiveness
C. Explosiveness
D. Toxicity

Answer 9

A. Temperature

Physical Properties - are properties
which can be measured without
changing the identity and composition
of a substance.
Examples: odor, color, density, boiling point, melting point, polarity, solubility,opacity, viscosity, etc.

Question 10

In order to decide whether a property is
chemical or physical, you must know
whether

A. measuring the property changes mass or
energy
B. the property is extensive or intensive
C. the property involves matter or energy
D. chemical or physical changes occur
when the property is measured

Answer 10

D. chemical or physical changes occur
when the property is measured

Physical Properties - are properties
which can be measured without
changing the identity and composition
of a substance.
Examples: odor, color, density, boiling point, melting point, polarity, solubility,opacity, viscosity, etc.
Chemical Properties - are properties that lead to changes in the identity and composition of a substance.
Examples: combustibility, pH, tendency
to rust, reaction with water, etc.

Question 11

A blue crystalline material is heated strongly in a test tube. A clear liquid condenses around the mouth of the tube and the crystals gradually lose their blue color and become white powder. Every gram of blue crystal
produces 0.36 g of clear liquid and 0.64 g of colorless powder. The same weight relationships are observed for samples of the crystals taken from many
different sources. These observations are consistent with the hypothesis that the blue crystals are:

A. Element
B. Compound
C. Solution
D. Heterogeneous mixture

Answer 11

B. Compound

Question 12

Smoke is an example of a/an

A. Homogenous mixture
B. Gaseous solution
C. Heterogeneous mixture
D. Compound

Answer 12

C. Heterogeneous mixture

Heterogeneous Mixture - mixture that
has distinguishable phases.
Homogenous Mixture - mixture that is uniform in appearance and has only one phase.
Compound - pure chemical substance
consisting of two or more different
elements that can be separated into
simpler substances by chemical means.
Solution - a homogenous mixture
composed of only one phase. Solutions
have particle sizes at the molecule or
ion level.

Question 13

Vanillin contains 63.15% C, 5.30% H,and 31.55% O whether it is extracted from vanilla beans, synthesized chemically from clove oils, or extracted from wood pulp wastes. Vanillin is most likely to be:

A. a heterogeneous mixture of elements
B. a compound of C, H, and o
C. a solution of C in H and o
D. a homogenous mixture of elements

Answer 13

B. a compound of C, H, and o

Compound - pure chemical substance
consisting of two or more different
elements that can be separated into
simpler substances by chemical means.
Heterogeneous Mixture - mixture that
has distinguishable phases.
Homogenous Mixture - mixture that is uniform in appearance and has only one phase.
Solution - a homogenous mixture
composed of only one phase. Solutions
have particle sizes at the molecule or
ion level.

Question 14

The meteorite ALH84001 contains tiny bubbles of gas trapped in the rock. The chemical composition of the gas in
these bubbles matches the composition
of the Martian atmosphere as
determined by Viking spacecraft in the 1970’s. The meteorite is an example of a/an

A. Binary compound
B. Element
C. Homogenous mixture
D. Heterogeneous mixture

Answer 14

D. Heterogeneous mixture

Heterogeneous Mixture - mixture that
has distinguishable phases.
Homogenous Mixture - mixture that is uniform in appearance and has only one phase.
Compound - pure chemical substance
consisting of two or more different
elements that can be separated into
simpler substances by chemical means.
Element - chemical substance that is
made up of a unique kind of atoms and
hence it cannot be broken down into
simpler substance. In total, 118
elements have been observed, 94 of
which occur naturally on Earth.

Question 15

A solid melts gradually between 85°C
and 95°C to give a milky, oily liquid.
When a laser beam shines through the
liquid, the path of the beam is clearly
visible. The milky liquid is likely to be:

A. An element
B. A compound
C. Solution
D. A heterogeneous mixture

Answer 15

D. A heterogeneous mixture

Heterogeneous Mixture - mixture that
has distinguishable phases.
Compound - pure chemical substance
consisting of two or more different
elements that can be separated into
simpler substances by chemical means.
Element - chemical substance that is
made up of a unique kind of atoms and
hence it cannot be broken down into
simpler substance. In total, 118
elements have been observed, 94 of
which occur naturally on Earth.
Solution - a homogenous mixture
composed of only one phase. Solutions
have particle sizes at the molecule or
ion level.

Question 16

Which of the following describes a
chemical change?

A. Sugar dissolving in a cup of coffee
B. Hamburger grease solidifying on a plate
C. Water boiling to form steam
D. Tarnishing silver

Answer 16

D. Tarnishing silver

A chemical change happens when one chemical substance is transformed into one or more different substances, such as when iron becomes rust. Chemical
changes occur through the process of chemical reactions, and the resulting substances have different properties
because their atoms and molecules are
arranged differently.

Question 17

Defined as dealing with the relations
between the physical properties of
substances and their chemical
formations along with their changes.

A. Inorganic Chemistry
B. Physical Chemistry
C. Organic Chemistry
D. Analytical Chemistry

Answer 17

B. Physical Chemistry

Physical Chemistry - defined as dealing with the relations between the physical properties of substances and their
chemical formations along with their
changes.
Organic Chemistry- branch of
chemistry deals with the chemistry of
carbon and living things.
Inorganic Chemistry - branch of
chemistry that deals with the structure
and interactions between inorganic
compounds, which are any compounds that are not based in carbon-hydrogen bonds.
Analytical Chemistry - branch of
chemistry involved with studying the properties of materials or developing tools to analyze materials.

Question 18

Who discovered plasma in 1879?

A. William Crookes
B. Irving Langmuir
C. Antoine Lavoisier
D. John Dalton

Answer 18

A. William Crookes

Plasma is an ionized gas that exist at
temperatures starting at several
thousand degrees Celsius. It was
discovered by Sir William Crookes in
1879 but, the term “plasma” was coined
by Irving Langmuir in 1928.

Question 19

Heterogeneous fluid containing solid particles that are sufficiently large for sedimentation:

A. Compound
B. Solution
C. Suspension
D. Colloid

Answer 19

C. Suspension

Types of Mixtures
1. Solution - a homogenous mixture
composed of only one phase. Solutions
have particle sizes at the molecule or
ion level.
2. Suspension - heterogeneous fluid
containing solid particles that are
sufficiently large for sedimentation.
3. Colloid - consist of microscopic
particles dispersed in a solvent. The
particles of colloids are larger than the
size of a molecule but smaller than
particles that can be seen with the
naked eye.

Question 20

When two liquids do not form a solution,
the two liquids are said to be

A. Miscible
B. Heterogeneous
C. Immiscible
D. Always acids

Answer 20

C. Immiscible

When two liquids do not form a solution,the two liquids are said to be like oil and water.

Question 21

Atoms of an element having same atomic number but different mass numbers are called

A. Isobars
B. Isotopes
C. Homologues
D. Isotones

Answer 21

B. Isotopes

Isotopes - atoms with the same
number of protons but different number
of neutrons. Example: Carbon-12 and
Carbon-13.
Isotones - atoms with same number of
neutrons but different number of
protons. Example: Boron-12 and
Carbon-13.
Isobars - atoms with the same mass number but different atomic number.Example: Carbon-12 and Boron-12.

Question 22

Atoms with same number of neutrons
but different number of protons:

A. Homologues
B. Isobars
C. Isotopes
D. Isotones

Answer 22

D. Isotones

Isotones - atoms with same number of
neutrons but different number of
protons. Example: Boron-12 and
Carbon-13
Isobars - atoms with the same mass number but different atomic number.Example: Carbon-12 and Boron-12.
Isotopes - atoms with the same
number of protons but different number
of neutrons. Example: Carbon-12 and
Carbon-13.

Question 23

The net electrical charge of an atom
under normal state is:

A. positive
B. infinite
C. neutral
D. negative

Answer 23

C. neutral

The net electrical charge of an atom
under normal state is neutral. Atoms or molecules with net electrical charge are called ions.

Question 24

The scientist who gave us the billiard
ball model of an atom:

A. E. Rutherford
B. J. Dalton
C. J. J. Thomson
D. N. Bohr

Answer 24

B. J. Dalton

John Dalton’s Atomic Model
-Known as the Billiard Ball model
-All matter is made of atoms
- Each element has different atoms.
- Atoms of different elements combine
in constant ratios to form compounds.

Question 25

The charge of electron was experimentally discovered by A. Millikan B. Goldstein C. Chadwick D. Thomson

Answer 25

A. Millikan Electron was discovered by J. J. Thomson in 1897 when he was studying the properties of cathode ray. In 1909, Robert Millikan and Harvey Fletcher conducted the oil drop experiment to determine the charge of an electron. They calculated this value to be 1.5924 × 10-19Coulombs (C), which is within 1% of the currently accepted value of 1.602176487 x10-19 C.

Question 26

Which types of ions metals form when they enter into a chemical reaction? A. Either positive or negative ions B. Positive ions C. Negative ions D. They do not form any ions

Answer 26

B. Positive ions Metals have less than 4 valence electrons. It is easier for most metals to give off their excess electrons when they form bonds with other atoms. Cation is an atom or molecule that lost an electron to become positively charged.

Question 27

"When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers" is a statement of: A. Law of Multiple Proportion B. Law of Definite Proportion C. Proust's Law D. Law of Conservation of Mass

Answer 27

A. Law of Multiple Proportion Law of Multiple Proportions (Dalton, 1766-1844): When elements A and B form a series of compounds, the ratio of masses of B that combine (in different compounds) with 1 gram of A can be reduced to small whole numbers. Conservation of Mass (Lavoisier,1743-1794): Mass can neither be created nor destroyed. Law of Definite Proportions (Proust, 1754-1826): A given compound always contains exactly the same proportion of elements by mass.

Question 28

The mass of a proton is _____ A. 9.1094 X10^-31 g B. 1.6726 X10^-24 g C. 1.6726 x 10^-27 g D. 1.6747 x10^-27g

Answer 28

B. 1.6726 X10^-24 g The mass of a proton is 1.6726 x 10^-27 kg or 1.6726 x10^-24 g.

Question 29

The mass of an electron is _____ A. 0.000549 amu B. 1.008665 amu C. 1.002722 amu D. 1.007277 amu

Answer 29

A. 0.000549 amu The mass of an electron is 9.1094 x 101-31 kg or 0.000549 amu. 1 atomic mass unit (amu) = 1.660538782x10 kg

Question 30

One amu is equal to _____ A. 1.6276 x10^-27 kg B. 6.2415 x10^18 kg C. 1.6749 x10^-27 kg D. 1.6605 x 10^-27 kg

Answer 30

D. 1.6605 x 10^-27 kg 1 atomic mass unit (amu) = 1.660538782x10 kg

Question 31

The mass of a neutron is equal to _____ A. All of these choices B. 1.6749 x10^-27 kg C. 1.6749 x10^-24 g D. 1.008665 amu

Answer 31

A. All of these choices The mass of a neutron is equal to 1.6749 x10^-27 kg or 1.008665 amu.1 atomic mass unit (amu) = 1.660538782x10 kg

Question 32

Proton was discovered by A. Ernest Rutherford B. J. J. Thomson C. James Chadwick D. John Dalton

Answer 32

A. Ernest Rutherford Protons were discovered by Ernest Rutherford in the year 1919, when he performed his gold foil experiment.

Question 33

The charge of a neutron is _____ A. None of these choices B. -1.6x10^-19 Coulomb C. 4.8 x 10^-10 Coulomb D. +1.6x10^-19 Coulomb

Answer 33

A. None of these choices The charge of neutron is 0. Neutron is neutral.

Question 34

An atom or molecule that lost an electron to become positively charged: A. Anion B. Polyatomic ion C. Cation D. Radical ion

Answer 34

C. Cation Cation is an atom or molecule that lost an electron to become positively charged. Anion is an atom or molecules that gained electrons and becomes negatively charged.

Question 35

Refers to the tendency of atoms to prefer to have eight electrons in the valence shell: A. Octet Rule B. Pauli's Exclusion Principle C. Hund's Rule D. Aufbau Principle

Answer 35

A. Octet Rule Octet rule - refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds Hund's Rule - states that every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied. Pauli's Exclusion Principle - states that no two electrons in an atom can have the set of quantum numbers. Aufbau Principle - electrons fill the orbital starting at the lowest possible energy states before filling higher states. This is used to determine the electron configuration of an atom, molecule or ion.

Question 36

"A given compound always contains exactly the same proportion of elements by mass" is a statement of: A. Law of Definite Proportion B. Law of Multiple Proportion C. Avogadro's Law D. Law of Conservation of Mass

Answer 36

A. Law of Definite Proportion Law of Definite Proportions (Proust, 1754-1826): A given compound always contains exactly the same proportion of elements by mass. Conservation of Mass (Lavoisier,1743-1794): Mass can neither be created nor destroyed. Law of Multiple Proportions (Dalton, 1766-1844): When elements A and B form a series of compounds, the ratio of masses of B that combine (in different compounds) with 1 gram of A can be reduced to small whole numbers.

Question 37

It is the energy change accompanying a mole of electrons being added to a mole of a gaseous atoms or ions. A. bingling energy B. fission C. electronic affinity D. biochemical energy

Answer 37

C. electronic affinity Electron affinity - describes the ability of an atom to accept an electron.

Question 38

A group of reactions where chain carriers are produced which by further reacting with the reactant produce back the chain carriers. A. Chain reaction B. Chain carrier C. Multiple reaction D. Consecutive reaction

Answer 38

A. Chain reaction A chemical chain reaction is a series of chemical reactions where the products of the reaction contribute to the reactants of another reaction.

Question 39

It is the scattering of light by colloidal particles A. Wolf Effect B. Tyndall Effect C. Mott Scattering D. Rayleigh Scattering

Answer 39

B. Tyndall Effect

Question 40

It is considered as derivatives of ammonia in which one or more of the hydrogen have been replaced by the alkyl or aryl group. It is characterized by unpleasant odors. A. Alkanes B. Amines C. Nitrites D. Esters

Answer 40

B. Amines

Question 41

______ involves the replacement of one of the atoms or groups of atoms attached to the carbon, "backbone" of the organic molecule. A. chemical reaction B. addition reaction C. substitution reaction D. halogenation

Answer 41

C. substitution reaction Single Displacement or Substitution Reaction - one element is displaced from a compound by another element.

Question 42

_____ states that in the addition of polar reagents to alkenes, the positive portion of the reagents adds to the carbon atom in the double bond that already has the most hydrogen atoms. A. Lock-and-key theory B. Markovnikou's rule C. Le Chatelier's principle D. Pauli Exclusion Theory

Answer 42

B. Markovnikou's rule Markovnikov's rule states that in an addition reaction of a protic acid HX (hydrogen chloride, hydrogen bromide, or hydrogen iodide) to an alkene or alkyne, the hydrogen atom of HX becomes bonded to the carbon atom that had the greatest number of hydrogen atoms in the starting alkene or alkyne. Le Chatelier's principle (also known as "Chatelier's principle" or "The Equilibrium Law") states that when a system experiences a disturbance (such as concentration, temperature, or pressure changes), it will respond to restore a new equilibrium state. Pauli's Exclusion Principle states that no two electrons in the same atom can have identical values for all four of their quantum numbers.

Question 43

In order to drive off carbon dioxide in a carbonate ore, one can use ____ A. diffraction B. combustion C. filtration D. calcination

Answer 43

D. calcination Calcination refers to heating a solid to high temperatures in absence of air or oxygen, generally for the purpose of removing impurities or volatile substances.

Question 44

It is required for organic compounds. A. C B. B C. H D. O

Answer 44

A. C Organic compound, any of a large class of chemical compounds in which one or more atoms of carbon are covalently linked to atoms of other elements.

Question 45

A buffer solution A. Changes pH only with the addition of a strong base B. Changes pH rapidly with the addition of an acid C. Resists changes in pH D. Does not change pH at all

Answer 45

C. Resists changes in pH Buffers are solutions that resist changes in pH, upon addition of small amounts of acid or base.

Question 46

It is the minimum amount of radioactive material needed to sustain a nuclear chain reaction. A. molar mass B. molecular mass C. atomic mass unit D. critical mass

Answer 46

D. critical mass The critical mass is the minimum amount of fissionable material needed to sustain a chain reaction. Molecular weight is the mass of a molecule of a substance. It can also be called molecular mass. The units for molecular weight are atomic mass units (amu). Molar mass is the mass of one mole of a substance. Molar mass is reported in grams per mole or g/mol.

Question 47

Electrons occupy all the orbitals of a given subshell singly before pairing begins. These unpaired electrons have parallel spins. This is known as: A. Building Up Principle B. David's Rule C. Aufbau Principle D. Hund's Rule

Answer 47

D. Hund's Rule Hund's Rule - states that every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied. Aufbau Principle - electrons fill the orbital starting at the lowest possible energy states before filling higher states. This is used to determine the electron configuration of an atom, molecule or ion.

Question 48

It is the calculation of both energy balances and material balances in a chemical system. A. stoichiometry B. molarity C. calorimetry D. molality

Answer 48

A. stoichiometry Stoichiometry is the calculation of reactants and products in chemical reactions in chemistry. Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products, leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers.

Question 49

It is an impure form of carbon, formed when coal is heated strongly in the absence of air. A. coke B. graphite C. austentite D. wrought carbon

Answer 49

A. coke Coke is an impure form of carbon formed when coal is heated strongly in the absence of air. It is widely used as a reducing agent in metallurgical operations. Graphite is a soft, black, slippery solid that has a metallic luster and conducts electricity. It consists of parallel sheets of carbon atoms. Austenite, also known as gamma-phase iron, is a metallic, non-magnetic allotrope of iron or a solid solution of iron, with an alloying element.

Question 50

It explains combustion as a result of loss of a substance. A. Phlogiston B. Reduction C. Roasting D. Fission

Answer 50

A. Phlogiston The phlogiston theory is a superseded scientific theory that postulated the existence of a fire-like element called phlogiston contained within combustible bodies and released during combustion.

Question 51

According to the Bronsted Theory, an acid is A. An electron donor B. A proton acceptor C. A proton donor D. An electron acceptor

Answer 51

C. A proton donor Bronsted-Lowry acid - any substance that donates hydrogen ion (proton). Bronsted-Lowry base - any substance that accepts hydrogen ion (proton).

Question 52

The energy possessed by a substance that allows it to be changed into a new substance. A. Physical energy B. Nuclear energy C. Chemical energy D. Potential energy

Answer 52

C. Chemical energy Chemical energy is the potential of a chemical substance to undergo a chemical reaction to transform into other substances. Some examples of storage media of chemical energy include batteries, food, and gasoline.

Question 53

The sugar of honey bee is composed of A. Sucrose and glucose B. Fructose and glucose C. Fructose and lactose D. Fructose and sucrose

Answer 53

B. Fructose and glucose Honey is composed mostly of the sugars glucose and fructose. It's what scientists term a supersaturated solution.

Question 54

How many valence electron(s) does a copper atom has? A. 4 B. 1 C. 3 D. 8

Answer 54

B. 1

Question 55

The two main parts of an atom are A. Nucleus and kernel B. Principal energy levels and energy sublevels C. Nucleus and energy levels D. Planetary electrons and energy levels

Answer 55

C. Nucleus and energy levels An atom is composed of two regions: the nucleus, which is in the center of the atom and contains protons and neutrons, and the outer region of the atom, which holds its electrons in orbit around the nucleus.

Question 56

A chemically reactive element that is the lightest in weight of all metals. A. Magnesium B. Hydrogen C. Lithium D. Beryllium

Answer 56

C. Lithium Under standard conditions, Lithium is the lightest metal and the lightest solid element. Like all alkali metals, lithium is highly reactive and flammable, and must be stored in mineral oil.

Question 57

Small amounts of acid that are secreted by cells in the lining of the stomach to aid in food digestion. A. Nitric acid B. Hydrochloric acid C. Carbonic acid D. Citric acid

Answer 57

B. Hydrochloric acid Stomach secretions are made up of hydrochloric acid, several enzymes, and a mucus coating that protects the lining of your stomach. Hydrochloric acid helps your body to break down, digest, and absorb nutrients such as protein.

Question 58

Chemical action may involve all of the following except: A. Breaking down compounds into elements B. Separation of the molecules in a mixture C. Reacting a compound and an element to form a new compound and a new element D. Combining of atoms of elements to form a molecule

Answer 58

B. Separation of the molecules in a mixture Chemical reaction, a process in which one or more substances, the reactants,are converted to one or more different substances, the products. Substances are either chemical elements or compounds. A chemical reaction rearranges the constituent atoms of the reactants to create different substances as products.

Question 59

To disperse fine particles of one substance evenly throughout another substance to create a state intermediate between a suspension and a solution. A. Colloid B. Diffusion C. Distribution D. Peptization

Answer 59

D. Peptization Peptization or Deflocculation is the process responsible for the formation of converting precipitate into colloid by shaking with it an electrolyte.

Question 60

When a substance is oxidized, it A. loses protons B. acts as a reducing agent C. acts as an oxidizing agent D. gains protons

Answer 60

B. acts as a reducing agent Oxidizing agent - a chemical substance that gives up oxygen or takes on electrons from another substance. Reducing agent - a chemical substance that takes on oxygen or gives up electrons to another substance.

Question 61

Which formula represents a salt? A. CH3COOH B. KCI C. CH3OH D. KOH

Answer 61

B. KCI Salts are ionic compounds that do not form OH- or H+ ions. KCI forms K+ and CI- ions. Therefore it is a salt.

Question 62

Which 0.1 M solution will turn phenolphthalein pink? A. LiOH(aq) B. HBr(aq) C. CO2(aq) D. CH30H(aq)

Answer 62

A. LiOH(aq) Phenolphthalein is often used as an indicator in acid-base titrations. For this application, it turns colorless in acidic solutions and pink in basic solutions. LiOH(aq) is a base and will turn phenolphthalein pink.

Question 63

When HCI(aq) is exactly neutralized by NaOH(aq), the hydrogen ion concentration in the resulting mixture is A. sometimes greater and sometimes less than the concentration of the hydroxide ions B. always greater than the concentration of the hydroxide ions C. always less than the concentration of the hydroxide ions D. always equal to the concentration of the hydroxide ions

Answer 63

D. always equal to the concentration of the hydroxide ions A neutralization reaction is also known as an acid-base neutralization reaction.In this reaction, acid and base reacts quantitatively to produce salt and water. The pH of the resulting product is 7 if both the acid and base are classified as strong acid and base. When HCI(aq) is exactly neutralized by NaOH(aq), the hydrogen ion concentration in the resulting mixture is always equal to the concentration of the hydroxide ions.

Question 64

In a fusion reaction, reacting nuclei must collide. Collisions between two nuclei are difficult to achieve because the nuclei are A. both negatively charged and repel each other B. oppositely charged and repel each other C. both positively charged and repel each other D. oppositely charged and attract each other

Answer 64

C. both positively charged and repel each other Collisions between two nuclei are difficult to achieve because the nuclei are... both positively charged and repel each other. In fusion light nuclei like hydrogen (deuterium) join to form heavier nuclei like helium. Because these nuclei are positively charged, they repel each other.

Question 65

What is the ratio of the number of moles per kilogram of solvent? A. formality B. molarity C. normality D. molality

Answer 65

D. molality Molality - the number of moles of solute per kilogram of solvent. Molarity - the number of moles of solute per liter of solution. Normality - expressed in gram equivalent weights of solute per liter of solution. Formality - the molecular weight in grams per liter of solution.

Question 66

What is the molecular weight in grams per liter of solution? A. formality B. molality C. normality D. molarity

Answer 66

A. formality Formality - the molecular weight in grams per liter of solution. Molality - the number of moles of solute per kilogram of solvent. Molarity - the number of moles of solute per liter of solution. Normality - expressed in gram equivalent weights of solute per liter of solution.

Question 67

It is expressed in gram equivalent weights of solute per liter of solution A. normality B. molarity C. molality D. formality

Answer 67

A. normality Normality- expressed in gram equivalent weights of solute per liter of solution. Formality - the molecular weight in grams per liter of solution. Molality - the number of moles of solute per kilogram of solvent. Molarity - the number of moles of solute per liter of solution.

Question 68

The dissolving medium in a solution is called A. water B. solvent C. solute D. acid

Answer 68

B. solvent Solvent - a substance in which another substance is dissolved, forming a solution. Solute - the substance being dissolved in another substance, usually the component of a solution in the lesser amount.

Question 69

The substance that losses electrons during an oxidation-reduction process A. reducing agent B. oxidizing agent C. solvent D. solute

Answer 69

A. reducing agent Oxidizing agent - a chemical substance that gives up oxygen or takes on electrons from another substance. Reducing agent - a chemical substance that takes on oxygen or gives up electrons to another substance.

Question 70

What is an ionized gas that exists at temperatures starting at several thousand degrees Celsius? A. Bose-Einstein condensate B. Filament C. None of these choices D. Plasma

Answer 70

D. Plasma Plasma is an ionized gas that exist at temperatures starting at several thousand degrees Celsius. It was discovered by Sir William Crookes in 1879 but, the term "plasma" was coined by Irving Langmuir in 1928. Bose-Einstein Condensate is a gaseous superfluid phase formed by atoms cooled to temperatures very near to absolute zero wherein the atoms slow down, combine and form a single entity called super atom.

Question 71

It is a gaseous superfluid phase formed by atoms cooled to temperatures very near to absolute zero A. Bose-Einstein condensate B. Filament C. Plasma D. Colloid

Answer 71

A. Bose-Einstein condensate Bose-Einstein Condensate is a gaseous superfluid phase formed by atoms cooled to temperatures very near to absolute zero wherein the atoms slow down, combine and form a single entity called super atom. Plasma is an ionized gas that exist at temperatures starting at several thousand degrees Celsius. It was discovered by Sir William Crookes in 1879 but, the term "plasma" was coined by Irving Langmuir in 1928

Question 72

State of matter that has definite volume but no definite shape A. Liquid B. Gas C. All of these choices D. Solid

Answer 72

A. Liquid Solid - has atoms or molecules that are closely packed. It has definite volume and shape. Liquid - has particles whose packing is between that of solid and gas. It has definite volume but no specific shape.Gas - has no definite volume or shape.It has particles that are comparatively separated

Question 73

It has atoms or molecules that are closely packed together A. Gas B. Solid C. Plasma D. Liquid

Answer 73

B. Solid Solid - has atoms or molecules that are closely packed. It has definite volume and shape. Liquid - has particles whose packing is between that of solid and gas. It has definite volume but no specific shape.Gas - has no definite volume or shape.It has particles that are comparatively separated

Question 74

Plasma naturally occurs in the form of A. Dry ice B. Lightning C. Smoke D. Dew

Answer 74

B. Lightning Plasma - an ionized gas that exist at temperatures starting at several thousand degrees Celsius. It occurs naturally in the form of stars and lightning.

Question 75

The ratio of the density of the substance to the density of some standard, usually water, is called A. Gauge pressure B. Specific gravity C. Mass density D. Specific volume

Answer 75

B. Specific gravity Specific Gravity or Relative Density is defined as the ratio of the density of a substance by the density of a standard substance. For solids and liquids, the reference is usually water; for gases, the reference is air.

Question 76

The darkest inner part of a shadow is called A. Nebula B. Umbra C. Regondula D. Penumbra

Answer 76

B. Umbra The umbra (Latin for "shadow") is the innermost and darkest part of a shadow, where the light source is completely blocked by the occluding body.

Question 77

It is a cloud of gases or dust in space A. Nebula B. Umbra C. Regondula D. Penumbra

Answer 77

A. Nebula A nebula is a giant cloud of dust and gas in space. Some nebulae come from the gas and dust thrown out by the explosion of a dying star, such as a supernova.

Question 78

Atoms with the same mass number but different atomic number are called A. Isotones B. Isobars C. Isotopes D. Isotropic

Answer 78

B. Isobars Isobars - atoms with the same mass number but different atomic number.Example: Carbon-12 and Boron-12. Isotopes - atoms with the same number of protons but different number of neutrons. Example: Carbon-12 and Carbon-13. Isotones - atoms with same number of neutrons but different number of protons. Example: Boron-12 and Carbon-13.

Question 79

What is the net electrical charge of an atom under normal state? A. Infinite B. Negative C. Positive D. Neutral

Answer 79

D. Neutral The net electrical charge of an atom under normal state is neutral. Atoms or molecules with net electrical charge are called ions.

Question 80

The substance that stimulates chemical reaction without being consumed in the reaction A. Emulsifier B. Product C. Reactant D. Catalyst

Answer 80

D. Catalyst Catalysts are substances that increase the reaction rate of a chemical reaction without being consumed in the process.A reactant is a substance that is present at the start of a chemical reaction. A product is a substance that is present at the end of a chemical reaction. An emulsifier is an additive which helps two liquids mix.

Question 81

In the periodic table, the atomic radius of the elements A. decreases from top to bottom and decreases from left to right B. decreases from top to bottom and increases from left to right C. increases from top to bottom and decreases from left to right D. increases from top to bottom and increases from left to right

Answer 81

C. increases from top to bottom and decreases from left to right (CHEM FIGURE)

Question 82

In the periodic table, electronegativity A. decreases from top to bottom and decreases from left to right B. decreases from top to bottom and increases from left to right C. increases from top to bottom and increases from left to right D. increases from top to bottom and decreases from left to right

Answer 82

B. decreases from top to bottom and increases from left to right

Question 83

What is the most abundant element in the Earth's crust? A. Oxygen B. Aluminum C. Silicon D. Nitrogen

Answer 83

A. Oxygen