Unit 2 College Chem

What are the two primary categories of energy?

Kinetic energy (energy of motion) and potential energy (stored energy).

How is kinetic energy (KE) calculated?

Using the formula KE = 1/2 mv², where m is mass and v is velocity.

What is the formula for gravitational potential energy (PE)?

PE = mgh, where h is height.

Give an example of a system where kinetic and potential energy transform.

A swinging pendulum.

In the context of a roller coaster, where is potential energy highest?

At the top of the roller coaster.

What wave properties characterize light?

Frequency (ν), wavelength (λ), and wavenumber (σ).

What is the relationship between speed of light, wavelength, and frequency?

c = λν, where c is the speed of light.

How is the energy of a photon related to its frequency?

The energy of a photon (E) is directly proportional to its frequency: E = hν.

What equation can be used to calculate the energy of a photon with a frequency of 5 x 10¹⁴ Hz?

E = (6.626 x 10⁻³⁴ J·s)(5 x 10¹⁴ Hz).

What does quantized energy refer to?

The discrete energy levels that electrons occupy in an atom.

What leads to the formation of bright line spectra in elements?

Transitions of electrons between energy levels, emitting or absorbing photons.

What does the Balmer series describe?

The visible spectral lines of hydrogen resulting from transitions to the n=2 energy level.

What is the Rydberg equation used for?

To calculate the wavelengths of spectral lines: 1/λ = R(1/n₁² - 1/n₂²).

What shape does an s orbital have?

Spherical.

How many types of atomic orbitals are there?

Four types: s, p, d, and f.

What is the maximum number of electrons an orbital can hold?

Each orbital can hold a maximum of 2 electrons.

How many orbitals does a p subshell contain?

Three orbitals.

What are the four quantum numbers used to describe atomic orbitals?

Principal (n), angular momentum (l), magnetic (ml), and spin (ms).

What does the Pauli Exclusion Principle state?

No two electrons in an atom can have the same set of four quantum numbers.

What does the Aufbau Principle dictate?

Electrons fill orbitals starting from the lowest energy level to the highest.

What does Hund’s Rule state about electron occupancy in degenerate orbitals?

Electrons will occupy degenerate orbitals singly before pairing up.

What is the electron configuration for carbon (atomic number 6)?

1s² 2s² 2p².

What trends are reflected in the organization of the periodic table?

Trends in atomic properties, including atomic radii, ionization energy, electron affinity, and metallic character.

How do atomic radii change across a period and down a group?

They decrease across a period and increase down a group.

What happens to ionization energy as you move across a period?

Ionization energy increases.

What is the trend for electron affinity across a period?

It generally becomes more negative.

How does metallic character change in the periodic table?

It increases down a group and decreases across a period.

What concept explains energy conservation in physical systems?

Understanding kinetic and potential energy.

What role does Planck's constant play in energy calculations?

It is used to calculate energy of photons (E = hν).

What is significant about the transition from n=3 to n=2 in hydrogen?

It produces a visible line in the spectrum.

What do quantum numbers help to understand?

Electron configurations and chemical bonding.

What physical system exemplifies potential energy at the top and kinetic energy at the bottom?

A roller coaster.

What is the term for the energy stored in springs?

Elastic potential energy.

What principle explains the order in which electrons fill orbitals?

The Aufbau Principle.

Define the term 'wavenumber'.

Wavenumber (σ) is defined as σ = 1/λ.

What system illustrates the transformation between kinetic and potential energy?

A swinging pendulum.

Why is understanding wave properties of light important?

It's vital for fields such as quantum mechanics and photonics.

How does adding electron shells affect atomic size?

It generally increases atomic size down a group.

What describes the energy levels of electrons in an atom?

Quantized energy.

What happens when electrons absorb or emit energy?

They transition between quantized energy levels.

What kind of trends can be observed in ionic and covalent bonding within the periodic table?

Attributes like electronegativity and atomic radius.

What determines the specific energy emitted or absorbed in transitions?

The difference in energy between quantized levels.

What is the outcome of electrons following Hund's Rule?

Minimization of electron-electron repulsion.

How are group trends in reactivity explained in terms of electron configuration?

By understanding their electron configurations and periodic trends.

What is the relationship of frequency and wavelength in determining the properties of light?

Higher frequency means shorter wavelength and vice versa.

How are atomic orbitals illustrated in the context of electron configuration?

They are depicted through subshell organization.