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Vocabulary Electron Configurati on Periodic Trends The Periodic Table Electroma gnetic Radiation Isoelectric ions and miscellane ous

Wavelength, frequency A 100

Distance between two wave peaks The number of waves that pass a given point per unit of time A 100

Photon, excited state A 200

Tiny packet of energy Contains an electron with excess energy A 200

Ground state, orbital A 300

Lowest possible energy state for an atom Region where an electron resides in an atom A 300

Pauli Exclusion Principle, Valence electrons A 400

An atomic orbital can hold no more than two electrons, and they must be of opposite spin Electrons in outermost (highest) occupied principal energy level A 400

Core electrons, Ionization energy A 500

Inner electrons of an atom Energy required to remove an electron from an atom in the gas phase A 500

Write the electron configuration for Al B 100

1s 2 2s 2 2p 6 3s 2 3p 1 B 100

Write the electron configuration for Ge B 200

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 2 B 200

Br, Bromine B 300

[Ar]4s 2 3d 10 4p 5 B 300

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 B 400

Fe, Iron B 400

Write the electron configuration for astatine B 500

[Xe] 6s 2 4f 14 5d 10 6p 5 B 500

Which of the following is the smallest atom? K, Ge, Si, O C 100

Oxygen, O C 100

Which of the following has the highest ionization energy? K, Ge, Si, O C 200

O

Which neutral atom has six 3d electrons? Fe, Co, Ru, Rh C 300

Fe C 300

Which one of the following elements has five valence electrons? B, C, N, F C 400

N

Use atomic structure to explain the trends of atomic size C 500

Atoms get bigger going down the periodic table and smaller going across the periodic table (across to the right). As you go down the periodic table the energy level increases, increasing the distance from the nucleus. Across the p.t., the energy level stays the same but the larger charge attracts the electrons making the distance smaller from the nucleus. C 500

What group are the alkali metals? D 100

Group 1 D 100

Where are the alkaline earth metals? D 200

Group 2 D 200

Where are the transition metal? D 300

Middle block on the periodic table; groups 3-12 D 300

Where are the halogens? D 400

Group 7 or 17 D 400

Where are the noble gases? D 500

Group 8 or 18 D 500

What would be the amount of energy contained by a photon whose frequency is 2.17 x Hz? E 100

1.44 x J E 100

What would be the wavelength of electromagnetic radiation (X- ray) if its frequency is 2.5 x Hz? E 200

1.2 x m E 200

What would be the energy of an FM radio signal if the wavelength is 1.5 m? E 300

1.33 x J E 300

As the wavelength of light increases, its frequency and energy do what? E 400

decrease E 400

What are the units of energy, frequency, wavelength and speed of light, respectively? E 500

J·s; Hz or s -1 ; m; m/s E 500

SOPHOMORES ONLY-What would be the electron configuration for the calcium ion, Ca +2 F 100

1s 2 2s 2 2p 6 3s 2 3p 6 F 100

What is the maximum number of electrons that can be in the third principal energy level? F 200

18 F 200

When an electron in an atom absorbs energy, it does what? F 300

Moves to a higher energy level F 300

In a hydrogen atom, an electron undergoing which of the following transitions would emit light of the shortest wavelength? from n=5 to n=1 From n=5 to n=2 From n=4 to n=1 From n=1 to n=5 F 400

From n=5 to n=1 Emitting energy means going from a higher energy level to lower energy level; shortest wavelength corresponds to highest energy change F 400

The 4 th energy level contains how many orbitals? F 500

4 or 16; 4 if you are talking s, p, d and f; 16 if you are thinking how many pairs of electrons total F 500

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