MTL 200 MIDTERM EXAM STUDY GUIDE ||
2025/2026 VERIFIED QUESTIONS & DETAILED
CORRECT ANSWERS || GUARANTEED PASS
<UPDATED>
6 properties of a solid material
1)Mechanical
2)Electrical
3)Thermal
4)Magnetic
5)Optical
6)Deterioration (chemical reaction)
Classification of Metals (5 types)
1)Composed of at least 1 metallic element
2)Atoms arranged orderly
3)Relatively Dense
4)Relatively Stiff and Strong
5)Good conductors of heat and electricity
Classification of Ceramics (4 types)
1) Compounds between metallic and nonmetallic elements
2) Commonly (oxides, nitrides, carbides)
3) Relatively stiff and strong
4)Very brittle (high susceptibility to fractures)
Classification of Polymers (6 types)
1)The family of plastic and rubbers
2)Large molecular structures
3)Can be ductile/pliable
4)Known to soften/decompose over time
,5)Low electric conductivity
6)Nonmegnetic
Classification of Composites (2 types)
1)Come from 2 or more types of material (metals, ceramics, polymers)
2)Designed to achieve multiple properties
Semiconductors
Both an insulator and a conductor
Electrons in Atoms
Electrons only have specific values of energy, if energy levels change, electrons must make a
quantum jump
How do electrons quantum jump? (2 points)
1)Either by absorbing energy and moving up
2)Or by releasing energy and moving down
Quantum Numbers (4 parameters to describe e)
1)Size
2)Shape
3)Spatial orientation
4)Probability density
Principle Quantum Number 1 (shell letter, and sub-shell)
Shell letter K
Sub-shell S
Principle Quantum Number 2 (shell letter, and sub-shell)
Shell letter L
Sub-shell s,p
Principle Quantum Number 3 (shell letter, and sub-shell)
Shell letter M
Sub-shell s,p,d
Principle Quantum Number 4 (shell letter, and sub-shell)
,Shell letter N
Sub-shell s,p,d,f
Electron Spin Movement
+1/2, -1/2
Ground State
electrons occupy all the lowest energy states
Hydrogen ground state
1s^1
Helium
1s^2
Sodium
1s^2,2s^2,2p^6,3s^1
Electropositive
elements capable of giving up electrons
Electronegative
elements ready to accept electrons
Bonding Energy
Eo=energy required to separate the atoms
The Primary Bond (3 types)
1)Ionic
2)Covalent
3)Metallic
Ionic Bonding (3 points)
1)The transfer of electrons
2)The attraction bonding forces are coulombic (positive-negative ions)
3)Nonderectional
Covalent bonding (3 points)
, 1)the share of electrons
2)directional
3)Non-metallic elements
Metallic Bonding (3 points)
1)Metals and alloys
2)electrons drift around through the solid
3)good at conducting heat and electricity
Secondary Bonds
Dipoles are the separation of a positive with a negative charge
Induced Dipole Bonds (4 points)
1)weakest secondary bonds
2)spacial distribution changes forming a small induced dipole between two atoms
3)Fluctuates
4)low bonding energies and melting points
Polar Molecule Induced Dipole Bond
Permanent dipole based on asymmetrical arrangement of charged atoms
Permanent Dipole Bonds (3 points)
1) Strongest
2)Hydrogen Bonding
3)High bonding energies and melting points
The structure of crystalline solids (3 types)
1)Crystalline
2)Amorphous
3)Lattice
Crystalline
Materials where atoms are situated in a repeating/periodic array over large atomic distances
Amorphous
Materials which don't crystallize
Lattice
2025/2026 VERIFIED QUESTIONS & DETAILED
CORRECT ANSWERS || GUARANTEED PASS
<UPDATED>
6 properties of a solid material
1)Mechanical
2)Electrical
3)Thermal
4)Magnetic
5)Optical
6)Deterioration (chemical reaction)
Classification of Metals (5 types)
1)Composed of at least 1 metallic element
2)Atoms arranged orderly
3)Relatively Dense
4)Relatively Stiff and Strong
5)Good conductors of heat and electricity
Classification of Ceramics (4 types)
1) Compounds between metallic and nonmetallic elements
2) Commonly (oxides, nitrides, carbides)
3) Relatively stiff and strong
4)Very brittle (high susceptibility to fractures)
Classification of Polymers (6 types)
1)The family of plastic and rubbers
2)Large molecular structures
3)Can be ductile/pliable
4)Known to soften/decompose over time
,5)Low electric conductivity
6)Nonmegnetic
Classification of Composites (2 types)
1)Come from 2 or more types of material (metals, ceramics, polymers)
2)Designed to achieve multiple properties
Semiconductors
Both an insulator and a conductor
Electrons in Atoms
Electrons only have specific values of energy, if energy levels change, electrons must make a
quantum jump
How do electrons quantum jump? (2 points)
1)Either by absorbing energy and moving up
2)Or by releasing energy and moving down
Quantum Numbers (4 parameters to describe e)
1)Size
2)Shape
3)Spatial orientation
4)Probability density
Principle Quantum Number 1 (shell letter, and sub-shell)
Shell letter K
Sub-shell S
Principle Quantum Number 2 (shell letter, and sub-shell)
Shell letter L
Sub-shell s,p
Principle Quantum Number 3 (shell letter, and sub-shell)
Shell letter M
Sub-shell s,p,d
Principle Quantum Number 4 (shell letter, and sub-shell)
,Shell letter N
Sub-shell s,p,d,f
Electron Spin Movement
+1/2, -1/2
Ground State
electrons occupy all the lowest energy states
Hydrogen ground state
1s^1
Helium
1s^2
Sodium
1s^2,2s^2,2p^6,3s^1
Electropositive
elements capable of giving up electrons
Electronegative
elements ready to accept electrons
Bonding Energy
Eo=energy required to separate the atoms
The Primary Bond (3 types)
1)Ionic
2)Covalent
3)Metallic
Ionic Bonding (3 points)
1)The transfer of electrons
2)The attraction bonding forces are coulombic (positive-negative ions)
3)Nonderectional
Covalent bonding (3 points)
, 1)the share of electrons
2)directional
3)Non-metallic elements
Metallic Bonding (3 points)
1)Metals and alloys
2)electrons drift around through the solid
3)good at conducting heat and electricity
Secondary Bonds
Dipoles are the separation of a positive with a negative charge
Induced Dipole Bonds (4 points)
1)weakest secondary bonds
2)spacial distribution changes forming a small induced dipole between two atoms
3)Fluctuates
4)low bonding energies and melting points
Polar Molecule Induced Dipole Bond
Permanent dipole based on asymmetrical arrangement of charged atoms
Permanent Dipole Bonds (3 points)
1) Strongest
2)Hydrogen Bonding
3)High bonding energies and melting points
The structure of crystalline solids (3 types)
1)Crystalline
2)Amorphous
3)Lattice
Crystalline
Materials where atoms are situated in a repeating/periodic array over large atomic distances
Amorphous
Materials which don't crystallize
Lattice
