MODULE 2

Question 1

occurs when an excess of a substance generated by human activity is present in the wrong environmental location.

Answer 1

Pollution

Question 2

mixture of gases that surrounds the Earth

Answer 2

Atmosphere

Question 3

mixture of gases that surrounds the Earth

Answer 3

Atmosphere

Question 4

Rigid shell of the Earth about 100km thick; thin surface forms the Earth’s crust

Answer 4

Lithosphere

Question 5

water portion of the biosphere

Answer 5

Hydrosphere

Question 6

What are the examples of natural pollution?

Answer 6

1. Volcanic Eruptions (Mt. Pinatubo)
2. Forest Fires
3. Smog (London, L.A.)

Question 7

What are examples of human-induced pollution?

Answer 7

1. Ozone Hole
2. Acid Rain
3. Coral Bleaching
4. Global Warming

Question 8

explains the properties and reactivities/stabilities of elements to form compounds.

Answer 8

Electronic Structure of Atoms

Question 9

Dalton’s Atomic Theory (1803-1807)

Answer 9

• All matter consist of tiny particles called atoms (molecules)
  1. Atoms are indestructible and unchangeable (false na)
  2. Elements are made up of the same kind of atoms (false na)
  3. Elements combine in simple whole number ratios (true)
  4. A chemical reaction involves rearrangement of atoms (true)

Question 10

_____________ discovered electrons in _____________ via _____________.

Answer 10

Thomson, 1990, cathode ray tube

Question 11

The Nobel Prize in Physics 1923 was awarded to _____________ for _____________.

Answer 11

Robert A. Milikan, his work on the elementary charge of electricity and on the photoelectric effect

Question 12

The Plum Pudding Model of Atom was developed by _____________ in _____________.

Answer 12

J.J. Thompson, 1904

Question 13

Sphere of positive charges where negative charges are embedded

Answer 13

Plum Pudding Model of Atom

Question 14

Majority of alpha particles penetrated the foil undeflected; some alpha particles experienced slight deflections; few (1 in 20,000) suffered serious deflections; few did not pass through the foil but bounced back in the direction from which they came.

Answer 14

Rutherford’s Observations

Question 15

The atom is mostly empty space, positive charge is concentrated in a very small volume; the mass of the atom is concentrated in a very small volume; the mass of the atom is concentrated in this volume

Answer 15

Nucleus

Question 16

This was awarded the Nobel Prize in Physics 1922 as it was developed in 1913, electrons in an atom move around the nucleus in circular orbits.

Answer 16

Bohr: Orbital Model

Question 17

This model has protons, neutrons, and electrons; electrons orbit around the nucleus which have protons and neutrons.

Answer 17

Bohr: Orbital Model

Question 18

same atomic number but different atomic masses

Answer 18

Isotopes

Question 19

This earned the Nobel Prize in Physics 1929; Developed by _________________ in _________________. He treated the electron as both wave and a particle.

Answer 19

Dual Nature of Electron; de Broglie, 1924

Question 20

This won the Nobel Prize in Physics 1932. This postulates that the position and energy (momentum) of an electron cannot be measured accurately at a given time; attributed to _________________.

Answer 20

Uncertainty Principle; Werner Heisenberg.

Question 21

They developed Schroedinger equation in _________________, based on quantum mechanics. They were awarded the Nobel Prize in Physics 1933 for _________________.

Answer 21

1933; the discovery of new productive forms of atomic theory

Question 22

pictorial representation of Schrodinger equation; each orbital contains 2 electrons.

Answer 22

Atomic orbitals

Question 23

order of orbitals (s,p,d,f)

Answer 23

AUFBAU principle

Question 24

In a given atom, no two electrons can have the same set of quantum numbers.

Answer 24

Pauli’s Exclusion Principle

Question 25

Electrons when distributed among the orbitals of the same energy will tend to distribute maximally among them.

Answer 25

Hund’s Rule of Maximum Multiplicity

Question 26

For _________________, the lowest energy is attained when the number of electrons with the same spin is maximized.

Answer 26

Degenerate orbitals

Question 27

What are the three ways of representing electron configurations?

Answer 27

1. Condensed spdf notation
2. Expanded spdf notation
3. Orbital designation

Question 28

What are the two magnetic properties of orbital pairs?

Answer 28

1. Paramagnetic
2. Diamagnetic

Question 29

unpaired electrons

Answer 29

Paramagnetic

Question 30

there are no unpaired electrons

Answer 30

Diamagnetic

Question 31

made the first table of elements

Answer 31

Antoine-Laurent Lavoisier

Question 32

developed the Law of Octaves

Answer 32

John H. Newlands

Question 33

developed the Law of Octaves

Answer 33

John H. Newlands

Question 34

arranged elements in order of increasing mass numbers

Answer 34

Dmitri Mendeleev

Question 35

assigned correct atomic numbers to the elements

Answer 35

Henry Moseley

Question 36

Modern Periodic Table is arranged ________________.

Answer 36

in order of increasing atomic number

Question 37

half the distance frpom its center of a like atom when these atoms are touching.

Answer 37

Atomic Size/Radius

Question 38

Energy required to remove an electron from its gaseous atom/ion.

Answer 38

Ionization Energy

Question 39

Energy evolved when an electron is added to a gaseous atom/ion.

Answer 39

Electron Affinity

Question 40

The ability of an atom to attract electrons to itself.

Answer 40

Electronegativity