Chemistry Flashcards

Question 1

Q

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

A

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

Q

Which of the following is an intensive
property?

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

Answer

A

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

Q

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

A

B. Deposition

(CHEM FIGURE)

Question 4

Q

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

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

Answer

A

D. Radius

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

Question 5

Q

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

A

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

Q

Which of the following is an extensive
property?

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

Answer

A

D. Volume

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

Question 7

Q

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

A

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

Q

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

A

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

Q

Which of the following is a physical
property?

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

Answer

A

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

Q

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

A

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

Q

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

A

B. Compound

Question 12

Q

Smoke is an example of a/an

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

Answer

A

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

Q

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

A

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

Q

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

A

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

Q

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

A

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

Q

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

A

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

Q

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

A

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

Q

Who discovered plasma in 1879?

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

Answer

A

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

Q

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

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

Answer

A

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

Q

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

A

C. Immiscible

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

Question 21

Q

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

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

Answer

A

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

Q

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

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

Answer

A

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

Q

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

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

Answer

A

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

Q

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

A

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

Q

The charge of electron was
experimentally discovered by

A. Millikan
B. Goldstein
C. Chadwick
D. Thomson

Answer

A

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

Q

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

A

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

Q

“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

A

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

Q

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

A

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

Q

The mass of an electron is _____

A. 0.000549 amu
B. 1.008665 amu
C. 1.002722 amu
D. 1.007277 amu

Answer

A

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

Q

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

A

D. 1.6605 x 10^-27 kg

1 atomic mass unit (amu) = 1.660538782x10 kg

Question 31

Q

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

A

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

Q

Proton was discovered by

A. Ernest Rutherford
B. J. J. Thomson
C. James Chadwick
D. John Dalton

Answer

A

A. Ernest Rutherford

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

Question 33

Q

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

A

A. None of these choices

The charge of neutron is 0. Neutron is
neutral.

Question 34

Q

An atom or molecule that lost an
electron to become positively charged:

A. Anion
B. Polyatomic ion
C. Cation
D. Radical ion

Answer

A

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

Q

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

A

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

Q

“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

A

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

Q

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

A

C. electronic affinity

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

Question 38

Q

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

A

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

Q

It is the scattering of light by colloidal
particles

A. Wolf Effect
B. Tyndall Effect
C. Mott Scattering
D. Rayleigh Scattering

Answer

A

B. Tyndall Effect

Question 40

Q

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

A

B. Amines

Question 41

Q

______ 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

A

C. substitution reaction

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

Question 42

Q

_____ 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

A

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

Q

In order to drive off carbon dioxide in a
carbonate ore, one can use ____

A. diffraction
B. combustion
C. filtration
D. calcination

Answer

A

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

Q

It is required for organic compounds.

A. C
B. B
C. H
D. O

Answer

A

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

Q

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

A

C. Resists changes in pH

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

Question 46

Q

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

A

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

Q

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

A

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

Q

It is the calculation of both energy
balances and material balances in a
chemical system.

A. stoichiometry
B. molarity
C. calorimetry
D. molality

Answer

A

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

Q

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

A

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

Q

It explains combustion as a result of
loss of a substance.

A. Phlogiston
B. Reduction
C. Roasting
D. Fission

Answer

A

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

Q

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

A

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

Q

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

A

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

Q

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

A

B. Fructose and glucose

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

Question 54

Q

How many valence electron(s) does a
copper atom has?

A. 4
B. 1
C. 3
D. 8

Question 55

Q

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

A

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

Q

A chemically reactive element that is
the lightest in weight of all metals.

A. Magnesium
B. Hydrogen
C. Lithium
D. Beryllium

Answer

A

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

Q

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

A

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

Q

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

A

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

Q

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

A

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

Q

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

A

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

Q

Which formula represents a salt?

A. CH3COOH
B. KCI
C. CH3OH
D. KOH

Answer

A

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

Q

Which 0.1 M solution will turn
phenolphthalein pink?

A. LiOH(aq)
B. HBr(aq)
C. CO2(aq)
D. CH30H(aq)

Answer

A

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

Q

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

A

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

Q

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

A

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.

Answer 64

A

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.

Answer 65

A

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.

Answer 66

A

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.

Answer 67

A

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.

Answer 68

A

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.

Answer 69

A

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.

Answer 70

A

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

Answer 71

A

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

Answer 72

A

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

Answer 73

A

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.

Answer 74

A

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.

Answer 75

A

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.

Answer 76

A

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.

Answer 77

A

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.

Answer 78

A

D. Neutral

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

Answer 79

A

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.

Answer 80

A

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

(CHEM FIGURE)

Answer 81

A

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

Answer 82

A

A. Oxygen

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