Chemistry class 11 , 12 notesEXAM WITH CORRECT
ACTUAL QUESTIONS AND CORRECTLY WELL DEFINED
ANSWERS LATEST ALREADY GRADED A+
Properties of Metals - ANSWER//Have 1-3 electrons in
the outer shell of each metal atom and lose electrons
readily Corrode easily (e.g., damaged by oxidation such
as tarnish or rust) Lose electrons easily Form oxides that
are basic Have lower electronegativities Physical
Properties of Nonmetals - ANSWER//Not lustrous (dull
appearance) Poor conductors of heat and electricity
Brittle solids May be solids, liquids or gases at room
temperature Transparent Chemical Properties of
Nonmetals - ANSWER//Usually have 4-8 electrons in
their outer shell Readily gain or share valence electrons
Form oxides that are acidic Have higher
electronegativities Alkali Metals - ANSWER//Group 1 (IA)
1 valence electron Explode when exposed to water Soft,
silver-coloured, solids at SATP react violently with water
to form basic solutions and liberate hydrogen gas
Alkaline Earth Metals - ANSWER//Group 2 (IIA) 2 valence
electrons Very reactive, solids at SATP form oxide
coatings when exposed to air Transition Metals -
ANSWER//Group 3-12 strong, hard metals wide range of
chemical and physical properties high melting points,
good conductors of electricity, variable reactivity
Halogens - ANSWER//Group 17 7 valence electrons
Highly reactive with alkali metals and alkaline earths
May be solids, liquids or gases at satp Not lustrous,
nonconductors of electricity Lanthanides -
ANSWER//Elements 57-70 (6th row) Silvery white
,metals that tarnish when exposed to air Reactive
Actinides - ANSWER//Elements 89-102 (7th row) All
radioactive Combine directly with most nonmetals
Noble Gases - ANSWER//Group 18 8 valence electrons
(complete valence shell) All gases at room temperature
Low melting and boiling points, very unreactive
Transuranic Elements - ANSWER//Elements that follow
uranium in the periodic table (93+) Representative
Element - ANSWER//An element in groups 1,2 and 13-18
Atomic Number (z) - ANSWER//The number of protons
in the nucleus Mass number (A) - ANSWER//The sum of
the number of protons and neutrons in the nucleus of
an atom Unified Atomic Mass Unit - ANSWER//A unit of
mass for atoms. 1/12 of the mass of a carbon-12 atom
Atomic mass (Ar) - ANSWER//The relative mass of an
atom on a scale on which the mass of one atom of
carbon-12 is exactly 12u. Approximately equivalent to
the mass number. Electron Arrangement - ANSWER//#of
protons; #of neutrons) # of e in first shell) # e in the
second shell) etc.) Nuclear Notation/Standard Atomic
Notation: AZX (can also be written without the Z or a as
X - A) Average Atomic Mass Formula - ANSWER//Aav =
A1 (%1/100) + A2 (%2/100) + ... *replace Aav with
atomic mass if they don't give you a value *replace A
with atomic number if they don't give you a value
Isotopes - ANSWER//Atoms that have the same number
of protons but different number of neutrons
Radioisotope - ANSWER//A radioactive isotope of an
element, occurring naturally or produced artificially
Radioactive - ANSWER//Capable of spontaneously
emitting radiation in the form of particles and/or
, gamma rays Trend - ANSWER//A gradual and consistent
change in the properties within periods or groups of the
periodic law Horizontal Period Trends - ANSWER//The
nuclear charge increases The shielding effect remains
constant (number of inner electrons stays the same) The
number of energy shells also stays the same The outer
electrons experience increasing nuclear attraction
Atomic radius goes down and increased attraction of
nucleus and valence electrons causes - Ionizing Energy
and Electronegativity to go up Increased electrons on
the outer shell means Electron affinity increases Vertical
Period Trends - ANSWER//The nuclear charge increase
BUT The shielding effect also increased The two cancel
each other out Since the number of electron shells
increases, the outer electrons are further from the
nucleus and experience decreasing nuclear attraction
Therefore the Atomic radius increases and the
decreasing attraction between the valence electrons
and the nucleus causes the Ionizing energy and the
Electronegativity to decrease. Electronic affinity
decreases down the family Trends in Metal Reactivity -
ANSWER//Left to right: more reactive Up: more reactive
Low ionization = high reactivity Trends in Non Metal
Reactivity - ANSWER//Left to right: more reactive Up:
more reactive High electron affinity = high reactivity
Electron Affinity - ANSWER//The energy change that
occurs when an electron is accepted by an atom in the
gaseous state Increases from left to right across the
periodic table Decreases from top to bottom down the
periodic table Electronegativity - ANSWER//The relative
ability of an atom, when bonded, to attract electrons
ACTUAL QUESTIONS AND CORRECTLY WELL DEFINED
ANSWERS LATEST ALREADY GRADED A+
Properties of Metals - ANSWER//Have 1-3 electrons in
the outer shell of each metal atom and lose electrons
readily Corrode easily (e.g., damaged by oxidation such
as tarnish or rust) Lose electrons easily Form oxides that
are basic Have lower electronegativities Physical
Properties of Nonmetals - ANSWER//Not lustrous (dull
appearance) Poor conductors of heat and electricity
Brittle solids May be solids, liquids or gases at room
temperature Transparent Chemical Properties of
Nonmetals - ANSWER//Usually have 4-8 electrons in
their outer shell Readily gain or share valence electrons
Form oxides that are acidic Have higher
electronegativities Alkali Metals - ANSWER//Group 1 (IA)
1 valence electron Explode when exposed to water Soft,
silver-coloured, solids at SATP react violently with water
to form basic solutions and liberate hydrogen gas
Alkaline Earth Metals - ANSWER//Group 2 (IIA) 2 valence
electrons Very reactive, solids at SATP form oxide
coatings when exposed to air Transition Metals -
ANSWER//Group 3-12 strong, hard metals wide range of
chemical and physical properties high melting points,
good conductors of electricity, variable reactivity
Halogens - ANSWER//Group 17 7 valence electrons
Highly reactive with alkali metals and alkaline earths
May be solids, liquids or gases at satp Not lustrous,
nonconductors of electricity Lanthanides -
ANSWER//Elements 57-70 (6th row) Silvery white
,metals that tarnish when exposed to air Reactive
Actinides - ANSWER//Elements 89-102 (7th row) All
radioactive Combine directly with most nonmetals
Noble Gases - ANSWER//Group 18 8 valence electrons
(complete valence shell) All gases at room temperature
Low melting and boiling points, very unreactive
Transuranic Elements - ANSWER//Elements that follow
uranium in the periodic table (93+) Representative
Element - ANSWER//An element in groups 1,2 and 13-18
Atomic Number (z) - ANSWER//The number of protons
in the nucleus Mass number (A) - ANSWER//The sum of
the number of protons and neutrons in the nucleus of
an atom Unified Atomic Mass Unit - ANSWER//A unit of
mass for atoms. 1/12 of the mass of a carbon-12 atom
Atomic mass (Ar) - ANSWER//The relative mass of an
atom on a scale on which the mass of one atom of
carbon-12 is exactly 12u. Approximately equivalent to
the mass number. Electron Arrangement - ANSWER//#of
protons; #of neutrons) # of e in first shell) # e in the
second shell) etc.) Nuclear Notation/Standard Atomic
Notation: AZX (can also be written without the Z or a as
X - A) Average Atomic Mass Formula - ANSWER//Aav =
A1 (%1/100) + A2 (%2/100) + ... *replace Aav with
atomic mass if they don't give you a value *replace A
with atomic number if they don't give you a value
Isotopes - ANSWER//Atoms that have the same number
of protons but different number of neutrons
Radioisotope - ANSWER//A radioactive isotope of an
element, occurring naturally or produced artificially
Radioactive - ANSWER//Capable of spontaneously
emitting radiation in the form of particles and/or
, gamma rays Trend - ANSWER//A gradual and consistent
change in the properties within periods or groups of the
periodic law Horizontal Period Trends - ANSWER//The
nuclear charge increases The shielding effect remains
constant (number of inner electrons stays the same) The
number of energy shells also stays the same The outer
electrons experience increasing nuclear attraction
Atomic radius goes down and increased attraction of
nucleus and valence electrons causes - Ionizing Energy
and Electronegativity to go up Increased electrons on
the outer shell means Electron affinity increases Vertical
Period Trends - ANSWER//The nuclear charge increase
BUT The shielding effect also increased The two cancel
each other out Since the number of electron shells
increases, the outer electrons are further from the
nucleus and experience decreasing nuclear attraction
Therefore the Atomic radius increases and the
decreasing attraction between the valence electrons
and the nucleus causes the Ionizing energy and the
Electronegativity to decrease. Electronic affinity
decreases down the family Trends in Metal Reactivity -
ANSWER//Left to right: more reactive Up: more reactive
Low ionization = high reactivity Trends in Non Metal
Reactivity - ANSWER//Left to right: more reactive Up:
more reactive High electron affinity = high reactivity
Electron Affinity - ANSWER//The energy change that
occurs when an electron is accepted by an atom in the
gaseous state Increases from left to right across the
periodic table Decreases from top to bottom down the
periodic table Electronegativity - ANSWER//The relative
ability of an atom, when bonded, to attract electrons
