SPLBE 2016 Flashcards
chemistry is derive from the Arabic word kimia meaning
alchemy
is the science that deals with the properties of organic and inorganic substances and their interactions with other organic and inorganic substances
chemistry
classification of matter by physical state:
solid, liquid, gas, plasma, bose-einstein condensate
rigidly structured materials having a fixed volume and shape
solid
has a fixed volume but assumes the shape of its container
liquid
most random state of matter, and has no fixed volume and either expands or contracts to fill its container completely
gas
is an ionize gas, a gas into which sufficient energy is provided to free electrons from atoms or molecules, to allow, ions and electrons, to exist
plasma
is a gaseous superfluid. it occurs at ultra-low temperature (very near to absolute zero), close to the point that the atoms are not moving at all
bose condensation
enumerate phase changes:
melting, freezing, sublimation, deposition, condensation, evaporation
is the process resulting in change of phase from a solid to a liquid
melting
another term for melting
fusion
is the phase change from liquid to solid
freezing
another term for freezing (phase change)
solidification
it is the transition from the solid to gas phase without passing the liquid state
sublimation
is a process in which gas transforms into solid
deposition
deposition (phase change) is also called as
desublimation
is the change in matter of a substance to a denser phase, such as a gas (or vapor) to a liquid
condensation
is the conversion of water from a liquid into gas
evaporation
two major changes in matter:
physical change and chemical change
no change in the basic composition or nature of matter
physical change
changing in the basic nature or composition into a new substance or material
chemical change
examples of physical change
melting, freezing, condensing, breaking, crushing, cutting and bending
examples of chemical change
digestion, respiration, photosynthesis, burning, rusting, decomposition….
properties of matter
physical and chemical, intensive and extensive
are properties which can be measured without changing the identity and composition of a substance
physical properties
examples of physical properties of matter
odor, color, density, boiling point, etc….
are properties that lead to changes in the identity and composition of a substance
chemical properties
examples of chemical properties
combustibility, flammability, toxicity, reactivity, acidity….
are those which do not depend on the size of he sample involved
intensive properties
example of intensive properties
density, boiling point, freezing point, color, melting point, taste, hardness, reactivity, luster, malleability and conductivity
are those that do depend on the size of the sample involved
extensive properties
examples of extensive properties
length, width, surface area, volume, mass, and weight
types of matter
pure substance, mixture
matter that has a definite composition and boiling point.
pure substance
are pure substance which cannot be broken down into simpler substances by ordinary chemical changes
elements
composed of two or more elements combined in a fixed proportion.
compounds
compounds can be broken down into simpler substances by _____
ordinary chemical reactions
elements are represented by
symbols
compounds are represented by
chemical formula
combination of two or more substances in no fixed proportions which can be separated by physical means
mixtures
constituents are not distinguishable even to some extent of magnification
homogenous mixture
constituents are readily visible or easily identifiable
heterogenous mixture
a collection of matter consisting of a positively charged core and maintains a number of electrons to balance the positive charge in the nucleus
atom
positively charged core
atomic nucleus
electron mass
9.1094E-28 g
electron charge
-1.602E-19 C
smallest particle in the atom
electron
proton mass
1.6726E-24g
proton charge
+1.602E-19
proton is _____ times the mass of the electron
1,837
neutron mass
1.6749E-24g
neutron charge
neutral
neutron is ______ times the mass of the electron
1,839
to find the maximum no. of electrons per shell:
2n^2
smallest known building block of matter
quark
up-quarks have electric charges of
+2/3
down quarks have charges of
-1/3
a proton is made up of
two up-quarks and a down-quark
is the smallest indivisible portion of a pure compound that retains a set of unique chemical properties.
molecule
consists of two or more atoms bonded together
molecule
molecules that contain one atom
monoatomic
molecules that contain two atoms
diatomic
molecules that contain three atoms
triatomic
molecules that contain more than one atom
polyatomic
the number of protons in the nucleus
atomic number(Z)
is approximately the sum of the number of protons and neutrons in the nucleus of the atom
atomic mass number
atomic mass number is the same as the
atomic weight(A)
one atomic mass unit is equivalent to
1/12 of the mass of an atom of Carbon 12 which is approx. equal to 1.66x10E-27 kg. This was formerly defined as 1/16 of the mass of one atom of oxygen 16
oxygen 16 is also called
Dalton, Da
the number of electrons in the outermost shell of an atom
valence
they strongly determine the electrical and thermal conductivity of the substance
valence
valence electrons that are less than 4 is considered as a
conductor
a semiconductor has how many valence electrons
4
how many valence electron does an insulator has
greater than 4
are formed when atoms gain or lose electrons
ions
are formed when a neutral atom loses electrons
cations
are formed when a neutral atom gains electrons
anions
tend to lose electrons to form positive ions
metallic atoms
tend to gain electrons to form negative ions
nonmetallic atoms
is an ion which has two negative charges on it
dianion
is an ion that contains an odd number of electrons and are mostly very reactive and unstable
radical ion
are polyatomic ions containing oxygen, such as carbonate and sulfate
oxyanions
the charge of an atom or ion is equal to
number of protons - number of electrons
are elements whose atoms have the same atomic number but different atomic weights.
isotopes
the nuclei of isotopes differ from one another only in the
number of neutrons
an isotope that is described as the heavy hydrogen
deuterium
an isotope of hydrogen that is radioactive
tritium
is the spontaneous disintegration of atomic nuclei (unstable nuclei) by the emission of radiation particles
radioactivity
what are the three radiation particles
alpha, beta, gamma
is a tabular method of displaying the chemical elements.
periodic table
the periodic table is first devise by
Dmitri Mendeleev
the periodic table is first devise in the year
1869
the periodic law states that
when the elements are arranged in the order of increasing atomic number, elements with similar properties appear at periodic interval
is a vertical column in the periodic table of the elements
groups or family
are considered the most important way of classifying the elements
groups
is a horizontal row in the periodic table of the elements
periods
define noble gases
all elements of group 8A have full valence shell. they do not need to react with other elements to attain a full shell, and are therefore unreactive, monoatomic gases
is the most inert element among noble gases
helium
inert means
lacking the ability to move
Group 8A is also called
Group 0 or Group 18 in the new concept
define halogens
aka group 7a elements are missing just one electron to fill their shell.
refers to the ability of an atom to attract shared electrons in a covalent bond
Electronegativity
in chemical reactions they tend to acquire electrons
halogens
properties of metals
luster, malleable and ductile, conduct heat and electricity, tend to lose electrons
able to be drawn out into a thin wire
ductile
properties of nonmetals
dull,
brittle,
do not conduct heat or electricity well,
tend to gain electrons
hard but liable to break or shatter easily
brittle
hard but liable to break or shatter easily
brittle
electronegativity is first proposed by
Linus Pauling
when was electronegativity proposed
1932
the most electronegative element; it pulls very strongly on the shared electrons in a covalent bond
flourine
ability of an atom to donate electrons
elecpositivity
for elements, it is the energy given off when an electron is added on the neutral atom.
electron affinity
refers to the measure of the willingness of an atom to receive an electron
electron affinity
is a measure of how much energy is required to remove an electron from a neutral atom
ionization energy
the measure of the tendency of an atom to resist the loss of electron
ionization energy
refers to the elements in a group
cogeners
law of conservation of mass
matter can neither be created nor destroyed
law of conservation of energy
energy cannot be created nor destroyed it can only be transformed from one form to another
law of definite composition
a pure compound is always made up of the same constituent elements combined in a definite proportion by weight
law of multiple proportion
when two elements react to form more than one compound, the different weights of the other are in the ratio of small whole numbers
is any compoun that dissociates in water into H+ ions
acids
is any substance that when dissolved in water, gives a solution a pH of less than 7
acids
the combination of H+ and water (H30+) is known as
arrhenius theory of acids
H30+ is known as
hydronium ion
is any compound that dissociates in water to yield an H+ ion
arrhenius acid
is any compound that is a proton donor when it dissolves in water
bronsted-lowry acid
is any compound that is an electron pair acceptor
lewis acid
properties of acids
- acids conduct electricity in aqueous solutions
- acids have a sour taste
- acids turn blue litmus paper to red
- acids have a ph between 0 and 7
- acids neutralize bases
- acids react with active metals to form hydrogen
- acids react with oxides and hydroxides of metals tot form salts and water
is any compound that dissociates in water into OH- ions.
bases
it is a chemical compound that absorbs hydronium ions when dissolved in water (a proton acceptor)
bases
is a special example of a base, where in an aqueous environment, hydroxide ions are donated
alkali
is any compound that dissociates in water to yield an OH- ion
arrhenius base
is any compound that is a proton acceptor when it dissolves in water
bronsted-lowry base
is any compound that is an electron pair donor
lewis base
properties of bases
- bases conduct electricity in aqueous solutions
- bases have a bitter taste
- bases turn red litmus paper to blue
- bases have a pH between 7 and 14
- bases neutralize acids, forming salts and water
the effect of an acid is to ______ in water, whereas bases _______
increase the hydronium ion concentration, reduce the concentration
pH stands for
power of hydrogen
is used to determine the number of hydrogen ions of a given substance.
pH
acids pH range from
5.0 and below
bases have a pH ranging from
8.5 and up
is a chemical compound in which ions are held together in a lattice structure by ionic bonds
ionic compounds
to form an ionic compound there needs to be atleast
one metal and one non-metal
in ionic compound, the metal element is usually the ____ charge and the non-metal element in a ____ charge
positive, negative
ionic compounds generally have high
melting and boiling points
ionic compounds have good electrical conductivity when
molten or in solution
when does ionic inorganic compounds form crystals
at room temperature, they become solids
is a term used or ionic compounds composed of the cations and anions
salt
why does salt need a positively charged cations and negatively charged anions
so that the product is neutral and without a net charge
solutions of salts in water are called
electrolytes
electrolytes as well as molten salts conduct
electricity
salt that does not contain a hydroxide ion or a hydrogen ion
normal salt
hydroxide ion
OH-
hydrogen ion
H+
is a salt that contain a hydroxide ion
basic salt
salts that contain a hydrogen ion
acidic salts
salts that contain a hydrogen ion
acidic salts
is a chemical compound of oxygen with other chemical elements
oxides
is a process by which one or more chemical substances are converted into one of more different chemical substances
chemical reaction
types of chemical reactions
- combination or synthesis
- decomposition or analysis
- single replacement
- double replacement or metathesis
what type of chemical reaction:
A + B –> AB
combination or synthesis
what type of chemical reaction:
A B —> A+B
decomposition or analysis
what type of chemical reaction:
A + BC —> AC + B
single replacement
what type of chemical reaction:
AB + XY —> AY + XB
double replacement or metathesis
is the math behind chemistry
stoichiometry
is used to calculate masses, moles and percent within a chemical equation
stoichiometry
the rules of determining stoichiometric relationships are based on
laws of conservation of mass and energy and the law of combining weights or volumes
a homogeneous mixture of two or more substances
solution
parts of solution
solute and solvent
the dissolved substance or the part that has a lesser amount
solute
the dissolving part of the solution or the part present in larger quantity
solvent
is the ability of a compound to dissolve in another compound
solubility
the measure of how much of a solute dissolves in a given amount of solvent
solubility
factors influencing solubility
- nature of solute and solvent
- temperature
- particle size of solid solute
are properties of a solution such as melting point and boiling point change when other compounds are added
colligative properties
colligative properties of solutions are properties that depend upon the
concentration of solute (molality)
measure of the number of moles of solute in a solution corresponding to 1 kg or 1000g of solvent
molality
factors that do not affect colligative properties
- size of particles
- mass of the particles
- type of particles
as the molality of the particles increases, it has the ff. effects on the solvent
- the vapor pressure decreases
- the boiling point increases
- the freezing point decreases
types of solution
saturated solution
unsaturated solution
supersaturated
dilute solution
concentrated solution
electrolyte
non-electrolyte
no more solute can dissolve in the given amount of solvent
saturated solution
the amount of solute dissolved in less than the solubility limit
unsaturated solution
contains dissolved amount of solute exceeding the normal solubility limit
supersaturated
comparatively has small amount of solute
dilute solution
relatively has larger amount of solute
concentrated solution
can conduct electricity, break into ions
electrolyte
a compound that will dissolve in water to form a solution that does not conduct electricity due to ions not being produced
non-electrolyte
are two liquids that do not dissolve in each other
immiscible liquids
are compound that dissolve easily in water
hydrophilic compounds
are compounds that do not dissolve easily in water
hydrophobic compounds
all nonpolar compounds such as hydrocarbons are _____
hydrophobic
is a measure of the quantity of an element or a compound.
mole
a mole of an element will have a mass equal to the element’s ________
atomic weight
a mole can be a
number quantity, a unit of mass, or a fixed volume of gas at STP
Avogadro’s number
6.022x10^23
a substance is numerically equal to its formula mass in grams
molar mass
a mole (mol) is defined as the number of atoms in exactly ___g of ____
12g of carbon-12
at stp, 1 mole of any gas occupies a volume of
22.4 L
mole formula
grams/molecular weight
1 mole is equal to _______ ions, atoms, molecules
6.022x10^23
1 mole is equal to ______ of an element or compound
molar mass
in a molecule or compound, it is the sum of the atomic weights of all the elements in the molecule
formula weight
is generally the same as the formula weight whose units are expressed as g/mole (or amu)
molecular weight
