Atomic Spectra Warm-Up, instruction, Assignment, and Quiz

Which of these statements correctly describe the atom? Check all that apply. All matter on Earth is made up of atoms. The subatomic particles of an element retain the properties of that element. The neutron has no charge and identifies the element. The electron is negatively charged and is located in a cloud surrounding the nucleus. The proton is positively charged and is found in the nucleus.

1, 4, & 5

Which statements accurately describe Ernest Rutherford's experiment? Check all that apply. The positively charged particles were deflected because like charges repel. The positively charged particles were deflected because opposite charges attract. The positively charged particles were deflected by the electron. The positively charged particles were deflected by the proton. The positively charged particles were deflected because the positive charge in the atom was concentrated. The positively charged particles were deflected because the positive charge in the atom was scattered throughout the atom.

1, 4, & 5

Which orbit has the highest energy?

3

Use the drop-down menus to show the development of the atomic theory from the oldest theory (1) to the most recent theory (5). Bohr: Dalton: Rutherford: Schrödinger and others: Thomson:

4 1 3 5 2

The table below shows the wavelengths of visible light that correspond to different colors. A student analyzes the emission spectrum of an unknown element and observes strong lines at the following wavelengths: 656 nm, 486 nm, 434 nm. Which absorption spectrum is the student most likely viewing?

A.

Which transition by an electron will release the greatest amount of energy? A B C D

A.

Whose atomic theory explains how atoms emit (release) and absorb light? Bohr's Dalton's Rutherford's Thomson's

A. Bohr's

Which statement is part of Bohr's atomic model? Electrons absorb or emit light when they change energy levels. Electrons with the highest energy are found with orbits of the smallest radius. Electrons exist as waves and clouds of probability with specific orbits and shapes. Electrons orbit the nucleus in narrow ellipses, like how the planets orbit the Sun.

A. Electrons absorb or emit light when they change energy levels.

What type of spectrum is shown below? absorption electromagnetic emission infrared light

A. absorption

Match each term with the appropriate definition absorption spectrum atomic spectrum spectroscopy emission spectrum

Absorption spectrum: represents energy absorbed as dark bands Atomic spectrum: represents energy emitted or absorbed during electron jumps Spectroscopy: the study of the absorption and emission of light by atoms Emission spectrum: represents energy absorbed as colored bands

Identify which type of scientist would use spectroscopy for each purpose. Identification of the composition of the sun and stars: Determination of chemical bonds: Prediction of the efficiency of possible laser materials: Identification of harmful bacteria in food and environmental samples:

An astronomer A chemist A physicist A biologist

Compare the spectra of mercury and sodium with the spectrum of an interstellar nebula. Most street lights are made from one of two elements—mercury or sodium. Explain why astronomers prefer that cities use sodium street lights instead of mercury street lights.

Astronomers prefer that cities use sodium street lights because the emission spectrum of sodium produces fewer lines than the emission spectrum of mercury. The emission spectrum of mercury causes interference, which can make it difficult to distinguish the emission spectra of astronomical objects.

This is the emission spectrum of aluminum. Which is the absorption spectrum of aluminum?

B.

What causes the appearance of lines in an emission spectrum? Light is absorbed as an electron moves to a higher energy state. Light is released as an electron moves to a lower energy state. An electron is released as light when it moves to a lower energy state. An electron is released as light when it moves to a higher energy state.

B. Light is released as an electron moves to a lower energy state.

Which statement accurately describes this atomic spectrum? The black lines represent the energy emitted by the electrons. The black lines represent the energy absorbed by the electrons. The colored lines represent the energy emitted by the electrons. The colored lines represent the energy absorbed by the electrons.

B. The black lines represent the energy absorbed by the electrons.

J.J. Thompson is credited with discovering the proton. electron. neutron. nucleus.

B. electron

Changes in the appearance of emission and absorption spectrums are caused by the activities of protons. electrons. neutrons. neutrinos.

B. electrons

An absorption spectrum of oxygen is shown below. What is most likely the emission spectrum of oxygen?

D.

Each element has its own emission and absorption lines. What is the best explanation for this? Each element has a specific number of protons and neutrons. Each element has a distinct number of electrons. Each element has a unique set of physical characteristics. Each element has unique energy levels.

D. Each element has unique energy levels.

Which best explains what happens when an electron moves from an excited state to the ground state? The electron absorbs energy as it moves to a lower energy level. The electron absorbs energy as it moves to a higher energy level. The electron releases energy as it moves to a higher energy level. The electron releases energy as it moves to a lower energy level.

D. The electron releases energy as it moves to a lower energy level.

This image shows a stream of positively charged particles being directed at gold foil. The positively charged particles are called "alpha particles" and each one is like a nucleus without any electrons. What is the best explanation for why a particle is striking point X? Alpha particles are mostly empty space, so they move in random directions, and one of these alpha particles can strike point X. The gold atoms contain negative electrons, so when alpha particles strike the gold they keep moving but in various directions. If an alpha particle hits the gold foil, a gold nucleus splits and a particle from it flies out at point X. When the dense, positive alpha particle passes close to a positive nucleus of gold, the alpha particle repels and hits the screen at point X.

D. When the dense, positive alpha particle passes close to a positive nucleus of gold, the alpha particle repels and hits the screen at point X.

If Thomson's atomic theory was accurate, what would the results of Rutherford's gold foil experiment have been?

If Thomson's atomic theory was accurate, the positively charged particles would have gone through the foil. The balanced positive charges and negative charges within the atom would have made the atom neutral, and the positive charges would not have been concentrated enough to cause deflection.

Match each scientist with the description of the appropriate atomic theory Thomson Dalton Rutherford Schrodinger and others Bohr

Thomson: Atoms contain electrons Dalton: Matter is made up of indivisible atoms Rutherford: The mass of an atom is concentrated in its center Schrodinger and others: Electrons exist in a cloud of probability Bohr: Electrons move in circular paths that have different energies

For each scenario, determine if the electron has absorbed energy or emitted energy. An electron jumps from n = 3 to n = 1. An electron jumps from n = 2 to n = 3. An electron jumps from n = 1 to n = 2. An electron jumps from n = 3 to n = 2.

emitted energy absorbed energy absorbed energy emitted energy