Chapter 5-Electrons and bonding Flashcards
What is the shell or energy level number also called?
The principle quantum number
How many electrons are there in the first 4 shells?
- 2
- 8
- 18
- 32
What did Shrodinger state about electrons?
They don’t move around in set paths around the nucleus-they instead behave as waves.
What do we call regions where electrons are most likely to occupy?
Orbitals
What are the 4 subshells?
S, P, D and F
How many electrons can an orbital hold and how do these electrons move?
2-with opposite spin
How many orbitals are in each subshell?
S-1
P-3
D-5
F-7
What is the shape of S orbitals?
Spherical
What is the shape of P orbitals?
Dumbell
How does the number of orbitals change as the shells increase.
The maximum orbital changes from S to P to D to F as the principle quantum number increases
What is the Aufbau princible?
Electrons are added one at a time to the lowest energy orbitals available until all in the atom are accounted for
What is the Pauli Exclusion principle?
An orbital can hold a maximum of 2 electrons and the 2 electrons have opposite spin
What is Hund’s rule?
Each orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin to minimise repulsion between electrons.
What is the order that subshells are filled in?
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d
What can we write as the shorthand notation for electron structure?
The noble gas in square brackets e.g. [Ne]
What are the blocks of the periodic table?
The highest energy subshell of an element
What are the 2 exceptions to the electron shell filling rules and what are their configurations?
- Chromium-[Ar] 4s¹ 3d⁵
- Copper-[Ar] 4s¹ 3D¹⁰
What rules do ions form in electron configuration and why?
Electrons from the 4s orbital are lost before those from the 3d orbital as the energy levels of the 3d orbital falls when it is full.
What is ionic bonding?
Attraction between all of the positive and all of the negative ions-attraction caused by electrostatic forces in all directions
What are the properties of ionic compounds?
- High melting and boiling point
- Strong electrostatic forces of attraction
- Oppositely charged ions that require lots of energy to overcome
- Can conduct electricity only in solution or molten
What can dissolve ionic compounds?
Polar solvents including parts that are δ⁺ and δ⁻
What does melting point of an ionic compound depend on?
- The charge-large electrostatic charge creates larger attraction
- The size of the ions-larger ions are further apart and forces are weaker
What is the formula for the melting point of an ionic compound?
F∝ (q₁q₂)/r²
What is covalent bonding?
Electrostatic attraction between the nucleus and shared pair of electrons
