Chemistry Flashcards
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
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.
Which of the following is an intensive
property?
A. Mass
B. Density
C. Volume
D. Number of atoms
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.
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
B. Deposition
(CHEM FIGURE)
Which of the following is an extensive
property of a bubble of air?
A. Temperature
B. Density
C. Percent oxygen
D. Radius
D. Radius
Extensive Properties - are properties that depend on the size of the sample involved.
Examples: volume, mass, weight, length,
etc.
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
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.
Which of the following is an extensive
property?
A. Color
B. Temperature
C. Melting point
D. Volume
D. Volume
Extensive Properties - are properties that depend on the size of the sample involved.
Examples: volume, mass, weight, length,
etc.
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
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.
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
B. total mg of caffeine
Extensive Properties - are properties that depend on the size of the sample involved.
Examples: volume, mass, weight, length,
etc.
Which of the following is a physical
property?
A. Temperature
B. Corrosiveness
C. Explosiveness
D. Toxicity
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.
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
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.
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
B. Compound
Smoke is an example of a/an
A. Homogenous mixture
B. Gaseous solution
C. Heterogeneous mixture
D. Compound
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.
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
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.
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
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.
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
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.
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
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.
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
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.
Who discovered plasma in 1879?
A. William Crookes
B. Irving Langmuir
C. Antoine Lavoisier
D. John Dalton
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.
Heterogeneous fluid containing solid particles that are sufficiently large for sedimentation:
A. Compound
B. Solution
C. Suspension
D. Colloid
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.
When two liquids do not form a solution,
the two liquids are said to be
A. Miscible
B. Heterogeneous
C. Immiscible
D. Always acids
C. Immiscible
When two liquids do not form a solution,the two liquids are said to be like oil and water.
Atoms of an element having same atomic number but different mass numbers are called
A. Isobars
B. Isotopes
C. Homologues
D. Isotones
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.
Atoms with same number of neutrons
but different number of protons:
A. Homologues
B. Isobars
C. Isotopes
D. Isotones
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.
The net electrical charge of an atom
under normal state is:
A. positive
B. infinite
C. neutral
D. negative
C. neutral
The net electrical charge of an atom
under normal state is neutral. Atoms or molecules with net electrical charge are called ions.
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
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.
The charge of electron was
experimentally discovered by
A. Millikan
B. Goldstein
C. Chadwick
D. Thomson
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.
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
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.
“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
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.
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
B. 1.6726 X10^-24 g
The mass of a proton is 1.6726 x 10^-27
kg or 1.6726 x10^-24 g.
The mass of an electron is _____
A. 0.000549 amu
B. 1.008665 amu
C. 1.002722 amu
D. 1.007277 amu
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
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
D. 1.6605 x 10^-27 kg
1 atomic mass unit (amu) = 1.660538782x10 kg
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
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
Proton was discovered by
A. Ernest Rutherford
B. J. J. Thomson
C. James Chadwick
D. John Dalton
A. Ernest Rutherford
Protons were discovered by Ernest
Rutherford in the year 1919, when he
performed his gold foil experiment.
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
A. None of these choices
The charge of neutron is 0. Neutron is
neutral.
An atom or molecule that lost an
electron to become positively charged:
A. Anion
B. Polyatomic ion
C. Cation
D. Radical ion
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.
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
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.
“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
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.
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
C. electronic affinity
Electron affinity - describes the ability
of an atom to accept an electron.
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
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.
It is the scattering of light by colloidal
particles
A. Wolf Effect
B. Tyndall Effect
C. Mott Scattering
D. Rayleigh Scattering
B. Tyndall Effect
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
B. Amines
______ 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
C. substitution reaction
Single Displacement or Substitution
Reaction - one element is displaced
from a compound by another element.
_____ 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
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.
In order to drive off carbon dioxide in a
carbonate ore, one can use ____
A. diffraction
B. combustion
C. filtration
D. calcination
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.
It is required for organic compounds.
A. C
B. B
C. H
D. O
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.
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
C. Resists changes in pH
Buffers are solutions that resist
changes in pH, upon addition of small
amounts of acid or base.
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
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.
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
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.
It is the calculation of both energy
balances and material balances in a
chemical system.
A. stoichiometry
B. molarity
C. calorimetry
D. molality
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.
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
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.
It explains combustion as a result of
loss of a substance.
A. Phlogiston
B. Reduction
C. Roasting
D. Fission
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.
According to the Bronsted Theory, an
acid is
A. An electron donor
B. A proton acceptor
C. A proton donor
D. An electron acceptor
C. A proton donor
Bronsted-Lowry acid - any substance
that donates hydrogen ion (proton).
Bronsted-Lowry base - any substance
that accepts hydrogen ion (proton).
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
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.
The sugar of honey bee is composed of
A. Sucrose and glucose
B. Fructose and glucose
C. Fructose and lactose
D. Fructose and sucrose
B. Fructose and glucose
Honey is composed mostly of the
sugars glucose and fructose. It’s what
scientists term a supersaturated
solution.
How many valence electron(s) does a
copper atom has?
A. 4
B. 1
C. 3
D. 8
B. 1
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
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.
A chemically reactive element that is
the lightest in weight of all metals.
A. Magnesium
B. Hydrogen
C. Lithium
D. Beryllium
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.
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
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.
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
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.
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
D. Peptization
Peptization or Deflocculation is the
process responsible for the formation of converting precipitate into colloid by shaking with it an electrolyte.
When a substance is oxidized, it
A. loses protons
B. acts as a reducing agent
C. acts as an oxidizing agent
D. gains protons
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.
Which formula represents a salt?
A. CH3COOH
B. KCI
C. CH3OH
D. KOH
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.
Which 0.1 M solution will turn
phenolphthalein pink?
A. LiOH(aq)
B. HBr(aq)
C. CO2(aq)
D. CH30H(aq)
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.
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
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.
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
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.
What is the ratio of the number of moles
per kilogram of solvent?
A. formality
B. molarity
C. normality
D. molality
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.
What is the molecular weight in grams
per liter of solution?
A. formality
B. molality
C. normality
D. molarity
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.
It is expressed in gram equivalent
weights of solute per liter of solution
A. normality
B. molarity
C. molality
D. formality
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.
The dissolving medium in a solution is called
A. water
B. solvent
C. solute
D. acid
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.
The substance that losses electrons
during an oxidation-reduction process
A. reducing agent
B. oxidizing agent
C. solvent
D. solute
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.
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
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.
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
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
State of matter that has definite volume
but no definite shape
A. Liquid
B. Gas
C. All of these choices
D. Solid
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
It has atoms or molecules that are
closely packed together
A. Gas
B. Solid
C. Plasma
D. Liquid
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
Plasma naturally occurs in the form of
A. Dry ice
B. Lightning
C. Smoke
D. Dew
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.
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
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.
The darkest inner part of a shadow is
called
A. Nebula
B. Umbra
C. Regondula
D. Penumbra
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.
It is a cloud of gases or dust in space
A. Nebula
B. Umbra
C. Regondula
D. Penumbra
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.
Atoms with the same mass number but
different atomic number are called
A. Isotones
B. Isobars
C. Isotopes
D. Isotropic
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.
What is the net electrical charge of an
atom under normal state?
A. Infinite
B. Negative
C. Positive
D. Neutral
D. Neutral
The net electrical charge of an atom
under normal state is neutral. Atoms or molecules with net electrical charge are called ions.
The substance that stimulates chemical reaction without being consumed in the reaction
A. Emulsifier
B. Product
C. Reactant
D. Catalyst
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.
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
C. increases from top to bottom and
decreases from left to right
(CHEM FIGURE)
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
B. decreases from top to bottom and
increases from left to right
What is the most abundant element in
the Earth’s crust?
A. Oxygen
B. Aluminum
C. Silicon
D. Nitrogen
A. Oxygen
