chapter 6

Question 1

Who was the primary contributor to the periodic table?

Answer 1

Dimitri Mendeleev (1837-1907) - chemist

Question 2

Who was the secondary contributor to the periodic table?

Answer 2

Henry Moseley (1887-1915) - physicist

Question 3

What contributions did Mendeleev make to the periodic table?

Answer 3

-elements were ordered by atomic mass
-saw repeating patterns of properties
-used pattern to predict undiscovered properties
-when atomic mass order did not fit other properties, he re-ordered by other properties

Question 4

What contributions did Moseley make to the periodic table?

Answer 4

-realized that the atomic number was more meaningful
-allowed for more accurate positioning of elements on the periodic table

Question 5

What was the periodic law?

Answer 5

when the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically

Question 6

______ summarize behavior

Answer 6

laws

Question 7

______ explains behavior

Answer 7

theories

Question 8

What was the importance of the periodic law?

Answer 8

it allows us to predict what the properties of an element will be based on its position on the table

Question 9

What are quantum mechanics?

Answer 9

its a theory that explains why the periodic trends in the properties exists (allows us to make predictions)

Question 10

Who was attributed to the periodic law?

Answer 10

Mendeleev

Question 11

What is the atomic radii property?

Answer 11

the physical size of an atom or ion (an estimated size)

Question 12

What is the ionization energy property?

Answer 12

the energy it takes to remove or expel an electron in the gas phases (form a cation)

Question 13

What is the electron affinity property?

Answer 13

the energy it takes to add an electron in the gas phases (form an anion)

Question 14

What happens to a elements radius as you go down the group? (up to down)

Answer 14

increase

Question 15

What happens to a element radius as you go across the period/row? (left to right)

Answer 15

decreases

Question 16

How does the radius decrease?

Answer 16

when electrons add to the same shell, there is pull or attraction that causes all the electrons to be closer to the nucleus; therefore, adding electrons causes the atomic radius to decrease

Question 17

What happens to cations in relation to the atomic radii property?

Answer 17

they lose electrons (positive charge) and decrease in atomic size (smaller

Question 18

What happens to anions in relation to the atomic radii property?

Answer 18

they gain electrons (negative charge) and increase in atomic size (larger)

Question 19

How do we make anions?

Answer 19

when an atom gains electrons (electron affinity)

Question 20

How do we make cations?

Answer 20

When an atom loses electrons (ionization energy)

Question 21

IE is endothermic T/F

Answer 21

true

Question 22

What happens to a elements ionization energy as you go down the group? (up to down)

Answer 22

decreases

Question 23

What happens to a elements ionization energy as you go across the period/row? (left to right)

Answer 23

increases

Question 24

electron affinity is exothermic- what does that mean

Answer 24

it’s usually a negative number

Question 25

What happens to a elements electron affinity as you go across the period/row? (left to right)

Answer 25

increases

Question 26

What are the three different types of thermal energy exchange?

Answer 26

endothermic, exothermic, enthalpy

Question 27

What are the two different types of energy from electrons exchange?

Answer 27

electricity, fireworks

Question 28

Why is direct observation of electrons within an atom impossible?

Answer 28

due to electrons being so small that they are unaffected by light

Question 29

Electrons behavior determines much of the behavior of ______

Answer 29

atoms

Question 30

What is the definition of light?

Answer 30

the form of electromagnetic radiation; type of energy in oscillating electric and magnetic fields

Question 31

What is the electric field?

Answer 31

a region where an electrically charged particle experiences a force

Question 32

What is a magnetic field?

Answer 32

a region where a magnetized particles experience a force

Question 33

What is wavelength?

Answer 33

the distance between adjacent crests or troughs in a wave; creates different colors

Question 34

What is frequency?

Answer 34

the number of complete wave passing during a point in a given period of time

Question 35

What makes amplitude different from wavelength?

Answer 35

amplitude changes the brightness

Question 36

What is spectra?

Answer 36

when atoms or molecules absorb energy, that energy is often released as energy (light)

Question 37

What is emission spectra?

Answer 37

when that emitted light is passed through a prism, a pattern of light is seen that is unique to that type of atom or molecule; two types

Question 38

what are the two types of emission spectra?

Answer 38

continuous, line

Question 39

What is an orbital?

Answer 39

a probability distribution map of regions within an atom where an electron is likely to be found

Question 40

the _____ the principle quantum number, the ____ the orbital shell and the _____ the energy level

Answer 40

higher; larger; higher

Question 41

What are the four different shapes or orbital subshells?

Answer 41

s-orbital, p-orbital, d-orbital, f-orbital

Question 42

What is paramagnetism?

Answer 42

when some atoms and ions will align (weak magnetism)

Question 43

What is ferromagnetism?

Answer 43

spins of unpaired electrons align in the same direction of the magnetic field

Question 44

How are ionic bonds classified?

Answer 44

a transfer of electrons of metals and nonmetals, 1.7+

Question 45

How are covalent bonds classified?

Answer 45

the sharing of electrons between nonmetals

Question 46

How are metallic bonds classified?

Answer 46

the pooling of electrons between metals

Question 47

What are valence electrons?

Answer 47

electrons in the outermost shell; shared in covalent compounds

Question 48

What ions are the easiest to remove?

Answer 48

valence electrons

Question 49

What is polarity?

Answer 49

unequal sharing of electrons

Question 50

What is electronegativity?

Answer 50

ability of an atom to attract electrons

Question 51

What is a resonance structure in chemistry?

Answer 51

Resonance structures are a group of two or more Lewis structures that represent ' electronic bonding

Question 52

What is the Heisenberg Uncertainty Principle?

Answer 52

it is impossible to determine simultaneously both the position and velocity of an electron or any other particle

Question 53

What is the Pauli Exclusion Principle?

Answer 53

no two electrons in the same atom can have the same set of four quantum numbers

Question 54

What is Hund's rule?

Answer 54

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Question 55

What is the octet rule?

Answer 55

Atoms tend to gain, lose or share electrons in order to have a full set of valance electrons.

Question 56

What is formal charge?

Answer 56

the charge associated with each bonded atom if all the electrons are shared equally

Question 57

the _shorter___ the bond, the ____ the bond

Answer 57

stronger

Question 58

what does nonpolar mean?

Answer 58

equal sharing of electrons

Question 59

What does polar mean?

Answer 59

unequal sharing of electrons

Question 60

What are columbic forces?

Answer 60

the attraction between a nucleus and an electron increases; with increasing magnitude of nuclear charge or atomic number

Question 61

What are the types of electron geometry?

Answer 61

Linear, Trigonal planar, Tetrahedral, Trigonal bipyromidal, octohedral

Question 62

What are the types of molecular geometry?

Answer 62

bent, square pyramidal, square planar, seesaw, T-shape, Linear