Exam 4 Flashcards
List out the order of electron configurations
1s²
2s²
2p⁶
3s²
3p⁶
4s²
3d¹⁰
4p⁶
5s²
4d¹⁰
5p⁶
6s²
What is a orbital diagram?
Numbers and arrows
how do you do noble gas notation?
Where are noble gasses?
Find the closest noble gas before your element on the periodic table.
Write its symbol in brackets [ ]
Continue the configuration from there
- have to pick up where left off in noble gas
(helium column)
What is the trend for ionization energy? and what is ionization energy?
Ionization energy is the energy required to remove an electron from a neutral atom in the gas phase.
↗ Increases across a period (left → right)
Why? More protons = higher nuclear charge = electrons held tighter Electrons are in the same shell, so the pull from the nucleus increases
↓ Decreases down a group (top → bottom)
Why? Electrons are farther from the nucleus (more shells) = weaker pull More shielding from inner electrons
what is atomic radius and whats the periodic trend?
It’s the distance from the nucleus to the outermost electron in an atom. Basically, how “big” the atom is.
➡️ Decreases across a period (left → right)
Why? More protons = stronger pull on electrons = electrons get pulled closer Even though electrons are being added, they’re added to the same energy level, so the atom shrinks
⬇️ Increases down a group (top → bottom)
Why? More energy levels = electrons farther from nucleus More electron shielding = less nuclear pull on outer electrons
What is electronegativity and whats the periodic trend for it?
Electronegativity is how strongly an atom pulls electrons toward itself in a chemical bond.
➡️ Increases across a period (left → right)
Why? More protons = stronger attraction to bonding electrons Atoms are closer to filling their valence shells, so they want electrons more
⬇️ Decreases down a group (top → bottom)
Why? More energy levels = electrons are farther from the nucleus = weaker pull Inner electrons shield the outer ones from nuclear charge
How does polarity work? (3)
- the more electronegative atom gets a partial negative charge
- the less electronegative atom gets a partial positive charge
- the greater the difference in electronegativity, the more polar the bond
What are the 3 main types of chemical bonds?
Ionic
nonpolar Covalent
polar covalent
What is an ionic bond?
A bond formed between a metal and a nonmetal where electrons are transferred.
What is a covalent bond?
A bond formed between nonmetals where electrons are shared.
Which type of bond is the strongest?
Dry state → Ionic > Polar Covalent
In water → Polar Covalent > Ionic (because ionic compounds often dissolve)
How can you tell if a bond is ionic?
Metal + Nonmetal
Large difference in electronegativity
What is a nonpolar covalent bond?
A bond where electrons are shared equally between atoms.
Occurs when atoms have similar or identical electronegativities.
What is a polar covalent bond?
A bond where electrons are shared unequally, causing a dipole (partial charges).
Occurs when there’s a moderate difference in electronegativity between atoms.
Whats wrong with boron?
Boron only needs 6 electrons
What does Boyle’s Law describe? and equation
Boyle’s Law: At constant temperature, pressure and volume are inversely related.
⬆️ Pressure = ⬇️ Volume (and vice versa)
Equation:
P₁V₁ = P₂V₂
What does Charles’s Law describe? and equation
Charles’s Law: At constant pressure, volume and temperature are directly related.
⬆️ Temperature = ⬆️ Volume
Equation:
V₁ / T₁ = V₂ / T₂
(T must be in Kelvin!)
What does Avogadro’s Law describe? and equation
Avogadro’s Law: At constant temperature and pressure, volume and moles are directly related.
⬆️ Moles (n) = ⬆️ Volume
Equation:
V₁ / n₁ = V₂ / n₂
What are the key conditions to remember for gas laws?
- Use Kelvin for all temperatures
- Keep units consistent
- Assume ideal gas behavior unless told otherwise
What are the standard units for STP (Standard Temperature and Pressure)?
Temperature: 273 K (0°C)
Pressure: 1 atm (also = 101.3 kPa or 760 mmHg)
Volume of 1 mole of gas: 22.4 L (at STP)
atm to mm
760
