Chem quiz unit2 Ultimate Study Guide

What is the speed of light in a vacuum?

$$c = 3.00 \times 10^8 \, \text{m} \, \text{s}^{-1}$$

What is the wave speed relation formula?

$c = \nu \times \beta$, where $\nu$ is frequency and $\beta$ is wavelength.

What is Planck's constant?

$$h = 6.63 \times 10^{-34} \, \text{J} \, \text{s}$$

How are wavelength and frequency related?

They are inversely related; as wavelength increases, frequency decreases.

What type of light has the longest wavelength?

Radio waves.

What is the visible spectrum range in nanometers?

Approximately $780 \, \text{nm}$ (red) to $380 \, \text{nm}$ (violet).

Define emission spectra.

Generated when excited electrons drop to lower energy levels, releasing photons.

What does the absorption spectrum demonstrate?

Dark gaps formed when cold vapor absorbs specific frequencies from continuous light.

What does the Heisenberg Uncertainty Principle state?

It is impossible to simultaneously know both the precise position and velocity of an electron.

What does the Aufbau principle state?

Electrons fill orbitals starting from the lowest energy levels.

What is the maximum number of electrons that can exist in a principal energy level n?

$2n^2$.

What is a principal quantum number ($n$)?

Positive integers indicating the main energy level of an electron.

What is the magnetic quantum number ($m_l$)?

Integers from $-l$ to $+l$ that describe the orientation of the orbital.

What is the difference between cations and anions?

Cations are positively charged and smaller than their parent atoms; anions are negatively charged and larger.

According to periodic trends, how does atomic radius change across a period?

It decreases from left to right due to increasing nuclear charge.

What is the reaction of alkali metals as you move down the group?

Reactivity increases down the group.

What is the first ionization energy?

The minimum energy required to remove one electron from a neutral gaseous atom.

What are the trends for ionization energy down a group?

It decreases down a group due to increased distance and shielding.

What phenomenon is observed in the line spectral series of Hydrogen when electrons drop to different energy levels?

Variety of emissions: UV (n=1), visible (n=2), and IR (n>=3).

How do electrons arrange themselves according to Hund's rule?

Each degenerate orbital is singly occupied with parallel spins before pairing.

What is the significance of the leap in ionization energy?

It indicates the removal of an electron from a complete inner noble gas core.

What is a key feature of transition metals in terms of electron configuration?

They often lose their outer $4s$ electrons before losing $3d$ electrons when forming ions.