electromagnetic radiation

Q: What are the three characteristics of a wave?

A: Wavelength, Frequency, Speed

Q: What is the relationship between wavelength and energy?

A: Long wavelength = low energy; Short wavelength = high energy

Q: What is a photon?

A: A quantum (packet) of electromagnetic energy

Q: What does it mean that energy is quantized?

A: It can only occur in discrete amounts (whole-number multiples of hv)

Q: What equation relates speed, wavelength, and frequency?

A: c = λν

Q: What is Planck’s constant?

A: 6.626 × 10⁻³⁴ J·s

Q: What equation gives the energy of a photon?

A: E = hv or E = hc/λ

Q: What does E = mc² relate?

A: Mass and energy

Q: What evidence supports electrons behaving as both particles and waves?

A: Electron diffraction and interference patterns

Q: What is an atomic emission spectrum?

A: Specific lines of color representing electrons falling to lower energy levels

Q: What is an absorption spectrum?

A: Spectrum with missing lines where light is absorbed to excite electrons

Q: How are flame tests used in identifying elements?

A: Each element emits a characteristic color when heated

Q: What is the Bohr model's main idea?

A: Electrons orbit the nucleus in fixed energy levels

Q: What happens when an electron jumps to a lower energy level?

A: It emits a photon of light

Q: What is the equation for energy transitions in hydrogen?

A: ΔE = 2.178 × 10⁻¹⁸ (1/n²final – 1/n²initial) J

Q: Why is the Bohr model limited?

A: It only works accurately for hydrogen-like atoms

Q: What do the bright lines in hydrogen's emission spectrum represent?

A: Specific energy drops (quantized transitions)

Q: What is the speed of light?

A: 3.00 × 10⁸ m/s