MTL 200 certification ASSESSMENT GUIDE
2025|MOST COMMON QUESTIONS WITH
CORRECTLY VERIFIED ANSWERS (the latest
ones)|ALREADY A+ GRADED|GUARANTEED
PASS/wishing you success in your studies
What are the three primary material eras? - Stone Age, Bronze Age, Iron Age
What are the four levels of Material Structures? - Subatomic Structures, Atomic
Structures, Micro structures, Macro structures
What are the three basic materials? - Metals, Ceramics and Polymers
Advanced Materials - semiconductors, biomaterials, smart materials, nanomaterials
atomic number - the number of protons in the nucleus of an atom, usually equals the
number of neutrons
Isotope - Atoms of the same element that have different numbers of neutrons
formula for atomic mass - Atomic Number + Neutrons
mole - the SI base unit used to measure the amount of a substance 6.022 x 10^23
Bohr's Atomic Model - Atoms have levels surrounding the nucleus where electrons are
found. Levels can hold different amounts of electrons depending on their distance from the
nucleus.
Wave-Mechanical Model [Schrodinger's Model] - Modern model of the atom, atoms have
electrons in "orbitals" that are like clouds around the nucleus
Quantum Numbers - A set of four numbers that specify the properties of atomic orbitals
and the properties of electrons in orbitals
Principal Quantum Number (n)
- symbolized by n, indicates the main energy level/shell occupied by the electron. N is
the row in the periodic table
, Secondary Quantum Number - symbol = l; tells which sublevel the electron is on and
determines the shape of the orbital; sublevels are repetitively numbered and also lettered
Valence Electrons - The electrons in the outermost shell, which participate in the bonding
between atoms.
Pauli Exclusion Principle - An atomic orbital may describe at most two electrons, each
with opposite spin direction
Bonding Energy - The energy required to separate two atoms that are chemically bonded
to each other to an infinite distance
What does a column group represent in a periodic table? - Similar valence electron
configurations/structure and chemical/physical properties
Electropositive Elements - The elements have a tendency to release valence electrons
(metals) and have a low electronegativity
Electronegative Elements - The elements having a tendency to accept valence electrons
(non-metals) and have a high electronegativity. [MC]
What is the general trend on the periodic table for increasing the Electronegativity? - The
electronegativity usually increases from left to right and bottom to top. [MC]
Ionic Bonding and Directonality - Chemical bonding that results from the electrical
attraction between cations and anions. Electron is given. Non-directional
Covalent Bonding and Directionality - Covalent Bonding happens when electrons are
shared between two atoms and they have a similar electronegativity.
Covalend Bonds are directional
Metallic Bonding and Directionality - In a metallic bond, the valence electrons are not
bound to a particular electron and can flow throughout the metal.
Metallic Bonds are non-directional.
Dipole - created by equal but opposite charges that are separated by a short distance
Fluctuating Induced Dipole Bonds - a fluctuating induced dipole bonds is a temporary
bond due to some atomic vibrations or motion.
Polar Molecule Induced Dipole Bonds - A polar molecule induced bond happens when
two polar molecules are attracted to their opposite sides. [Water Molecule]
2025|MOST COMMON QUESTIONS WITH
CORRECTLY VERIFIED ANSWERS (the latest
ones)|ALREADY A+ GRADED|GUARANTEED
PASS/wishing you success in your studies
What are the three primary material eras? - Stone Age, Bronze Age, Iron Age
What are the four levels of Material Structures? - Subatomic Structures, Atomic
Structures, Micro structures, Macro structures
What are the three basic materials? - Metals, Ceramics and Polymers
Advanced Materials - semiconductors, biomaterials, smart materials, nanomaterials
atomic number - the number of protons in the nucleus of an atom, usually equals the
number of neutrons
Isotope - Atoms of the same element that have different numbers of neutrons
formula for atomic mass - Atomic Number + Neutrons
mole - the SI base unit used to measure the amount of a substance 6.022 x 10^23
Bohr's Atomic Model - Atoms have levels surrounding the nucleus where electrons are
found. Levels can hold different amounts of electrons depending on their distance from the
nucleus.
Wave-Mechanical Model [Schrodinger's Model] - Modern model of the atom, atoms have
electrons in "orbitals" that are like clouds around the nucleus
Quantum Numbers - A set of four numbers that specify the properties of atomic orbitals
and the properties of electrons in orbitals
Principal Quantum Number (n)
- symbolized by n, indicates the main energy level/shell occupied by the electron. N is
the row in the periodic table
, Secondary Quantum Number - symbol = l; tells which sublevel the electron is on and
determines the shape of the orbital; sublevels are repetitively numbered and also lettered
Valence Electrons - The electrons in the outermost shell, which participate in the bonding
between atoms.
Pauli Exclusion Principle - An atomic orbital may describe at most two electrons, each
with opposite spin direction
Bonding Energy - The energy required to separate two atoms that are chemically bonded
to each other to an infinite distance
What does a column group represent in a periodic table? - Similar valence electron
configurations/structure and chemical/physical properties
Electropositive Elements - The elements have a tendency to release valence electrons
(metals) and have a low electronegativity
Electronegative Elements - The elements having a tendency to accept valence electrons
(non-metals) and have a high electronegativity. [MC]
What is the general trend on the periodic table for increasing the Electronegativity? - The
electronegativity usually increases from left to right and bottom to top. [MC]
Ionic Bonding and Directonality - Chemical bonding that results from the electrical
attraction between cations and anions. Electron is given. Non-directional
Covalent Bonding and Directionality - Covalent Bonding happens when electrons are
shared between two atoms and they have a similar electronegativity.
Covalend Bonds are directional
Metallic Bonding and Directionality - In a metallic bond, the valence electrons are not
bound to a particular electron and can flow throughout the metal.
Metallic Bonds are non-directional.
Dipole - created by equal but opposite charges that are separated by a short distance
Fluctuating Induced Dipole Bonds - a fluctuating induced dipole bonds is a temporary
bond due to some atomic vibrations or motion.
Polar Molecule Induced Dipole Bonds - A polar molecule induced bond happens when
two polar molecules are attracted to their opposite sides. [Water Molecule]
