Arrangement of electrons in an atom

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24 Terms

1

Who was the first scientist to provide a picture of the arrangement of the electrons in an atom?

Niels Bohr

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2

How is a continuous spectrum formed?

By shining white light through a prism and viewing it on a screen.

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3

What is an emission line spectrum?

A spectrum with a black background and colored lines on it.

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4

What does Bohr's Theory state about electrons?

Electrons revolve around the nucleus in fixed paths called orbits without gaining or losing energy when in these orbits.

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5

What happens to an electron when it absorbs energy according to Bohr's Theory?

It jumps to a higher energy level, known as the excited state.

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6

Why do electrons not remain in the excited state?

Because they are unstable and must return to their original ground state.

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7

Define the energy level.

The fixed energy value that an electron in an atom may have.

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8

Define ground state.

The state of an atom in which the electrons occupy the lowest available energy levels.

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9

Define excited state.

The state of an atom in which the electrons occupy higher energy levels than those available in the ground state.

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10

Where is the Lyman series located?

In the ultraviolet region, when an electron falls to the n=1 energy level.

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11

Where is the Paschen series located?

In the infrared region, when an electron falls to the n=3 energy level.

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12

What is the name of the series of lines in the visible spectrum?

The Balmer series, when the electron falls to the n=2 energy level.

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13

In the formula E=hf, what do h and f stand for?

h = Planck's constant, f = frequency of light.

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14

What is Atomic Absorption Spectrometry?

A technique where white light is passed through a gas sample of an element before going through a prism, discovering dark lines in the continuous spectrum.

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15

Give 2 uses for Emission line spectrum and Atomic Absorption Spectrometry.

Emission: identification of elements and used in fireworks; Absorption: identification of elements and finding the concentration of elements.

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16

What are energy sublevels?

Subdivisions of a main energy level consisting of one or more orbitals of the same energy.

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17

Why does the 4s sublevel come before the 3d sublevel?

Because it takes more energy to get into the 3d sublevel.

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18

Who discovered that electrons travel in a wave motion?

De Broglie.

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19

What is Heisenberg’s Uncertainty Principle?

It states that it is impossible to measure both the velocity and position of an atom at the same time.

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20

Give 3 limitations of Bohr’s theory.

It only works for hydrogen, did not consider the wave nature of electrons, and did not address sublevels.

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21

Define an atomic orbital.

A region in space where there is a high probability of finding an electron.

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22

What shape is the S orbital?

Spherical.

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23

What shape are the P orbitals?

Dumbbell shape.

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24

How were energy sublevels discovered?

Scientists found that the emission lines were not singular, but some were made of multiple lines.

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