Chemistry Final Exam Study

Front 1

How is error calculated?

Back 1

Error = experimental value - accepted value

Front 2

How is percent error calculated?

Back 2

Percent error = |error|/accepted value x100%

Front 3

How is degrees Kelvin taken from degrees Celsius?

Back 3

K = C + 273

Front 4

First to suggest that atoms existed. Believed that they were both invisible and indestructible.

Back 4

Democritus

Front 5

Modernized information about atoms, and created a set of theories to help explain them.

Back 5

Dalton

Front 6

First to discover the existence of a negatively charged atomic particle, today known as an electron.

Back 6

Thomson

Front 7

Discovered the charge of an electron, as well as its mass relative to that of a hydrogen atom.

Back 7

Millikan

Front 8

Mass of an electron relative to that of a hydrogen atom.

Back 8

1/1840

Front 9

First to discover the existence of a positively charged atomic particle, today known as an proton.

Back 9

Goldstein

Front 10

First to discover the existence of a neutral particle, today known as an neutron.

Back 10

Chadwick

Front 11

Proposed that an atom is mostly empty space, and then each has a nucleus.

Back 11

Rutherford

Front 12

What could Rutherford's atomic model not explain?

Back 12

The chemical properties of elements.

Front 13

How is the number of neutrons in an element calculated?

Back 13

Neutrons = mass number - atomic number

Front 14

Proposed that electrons move in fixed paths about the nucleus of an atom.

Back 14

Bohr

Front 15

Principle that states that electrons occupy the orbitals of lowest energy first.

Back 15

Aufbau Principle

Front 16

According to this, an atomic orbital may, at most, have two electrons spinning in opposite directions.

Back 16

Pauli Exclusion Principle

Front 17

Idea that electrons occupy energy levels in such a way that an energy level is filled entirely by electrons of the same direction of spin.

Back 17

Hund's Rule

Front 18

How is wavelength and frequency calculated?

Back 18

The speed of light = wavelength x frequency

Front 19

What is the speed of light?

Back 19

2.998 x 10 to the 8 meters per second

Front 20

What is Avogadro's constant?

Back 20

6.02 x 10 to the -23

Front 21

Arranged the elements in a new periodic table in order of mass.

Back 21

Mendeleev

Front 22

Grouped elements into triads in order to sort them by their chemical properties.

Back 22

Dobereiner

Front 23

What is the periodic trend for atomic mass?

Back 23

Increases down, decreases across.

Front 24

What is the periodic trend for ionization energy?

Back 24

Increases down, increases across.

Front 25

What is the periodic trend for electronegativity?

Back 25

Decreases down, increases across.

Front 26

What is the periodic trend for nuclear charge?

Back 26

Increases down, increases across.

Front 27

What is the periodic trend for shielding?

Back 27

Increases down, remains constant across.

Front 28

What is the periodic trend for ionic size?

Back 28

Increases down, decreases across.

Front 29

What is electronegativity?

Back 29

The ability of an atom to attract electrons when the atom is in a compound.

Front 30

What is first ionization energy?

Back 30

The energy required to remove an electron from an atom.

Front 31

Atoms tend to gain or lose electrons in order to achieve a noble gas structure by the _______.

Back 31

Octet rule

Front 32

If the components of an alloy are relatively the same size, what kind of alloy is formed?

Back 32

Substitutional alloy

Front 33

What are the three metallic crystallization patterns?

Back 33

Body-centered cubic, face-centered cubic, and hexagonal close-packed.

Front 34

If the components of an alloy are relatively different in size, what kind of alloy is formed?

Back 34

Interstitial alloy

Front 35

Theory that states the the repulsion between electrons causes molecular shapes to change in a way that leaves the electrons as far apart as possible.

Back 35

VSEPR (Valence-Shell Electron-Pair Repulsion) Theory

Front 36

Bond angle of linear triatomic.

Back 36

180 degrees.

Front 37

Bond angle of trigonal planar.

Back 37

120 degrees.

Front 38

Bond angle of bent triatomic.

Back 38

105 degrees.

Front 39

Bond angle of pyramidal.

Back 39

107 degrees.

Front 40

Bond angle of tetrahedral.

Back 40

109.5 degrees.

Front 41

The two weakest attractions between molecules belong in this collective category.

Back 41

Van der Waals forces

Front 42

Weakest of all molecular attractions. Caused by the motion of electrons.

Back 42

Dispersion forced

Front 43

Molecular attractions caused by the attraction between polar molecules.

Back 43

Dipole-dipole interactions

Front 44

Attractive forces in which hydrogen bonds to an electronegative atom and an unshared electron pair of electrons from another electronegative atom.

Back 44

Hydrogen bonds

Front 45

If hydrogen bonds with any of these elements, then a hydrogen bond is present.

Back 45

Nitrogen, oxygen, and fluorine.

Front 46

Why are the properties of network solids superior to those of typical solids?

Back 46

Melting or breaking down a network solid would requite breaking down the covalent bonds throughout it.