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Chem 1201 > chapter 6 > Flashcards

chapter 6 Flashcards

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1
Q

Who was the primary contributor to the periodic table?

A

Dimitri Mendeleev (1837-1907) - chemist

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2
Q

Who was the secondary contributor to the periodic table?

A

Henry Moseley (1887-1915) - physicist

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3
Q

What contributions did Mendeleev make to the periodic table?

A

-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

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4
Q

What contributions did Moseley make to the periodic table?

A

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

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5
Q

What was the periodic law?

A

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

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6
Q

______ summarize behavior

A

laws

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7
Q

______ explains behavior

A

theories

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8
Q

What was the importance of the periodic law?

A

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

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9
Q

What are quantum mechanics?

A

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

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10
Q

Who was attributed to the periodic law?

A

Mendeleev

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11
Q

What is the atomic radii property?

A

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

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12
Q

What is the ionization energy property?

A

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

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13
Q

What is the electron affinity property?

A

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

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14
Q

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

A

increase

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15
Q

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

A

decreases

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16
Q

How does the radius decrease?

A

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

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17
Q

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

A

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

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18
Q

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

A

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

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19
Q

How do we make anions?

A

when an atom gains electrons (electron affinity)

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20
Q

How do we make cations?

A

When an atom loses electrons (ionization energy)

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21
Q

IE is endothermic T/F

A

true

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22
Q

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

A

decreases

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23
Q

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

A

increases

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24
Q

electron affinity is exothermic- what does that mean

A

it’s usually a negative number

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25
Q

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

A

increases

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26
Q

What are the three different types of thermal energy exchange?

A

endothermic, exothermic, enthalpy

27
Q

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

A

electricity, fireworks

28
Q

Why is direct observation of electrons within an atom impossible?

A

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

29
Q

Electrons behavior determines much of the behavior of ______

A

atoms

30
Q

What is the definition of light?

A

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

31
Q

What is the electric field?

A

a region where an electrically charged particle experiences a force

32
Q

What is a magnetic field?

A

a region where a magnetized particles experience a force

33
Q

What is wavelength?

A

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

34
Q

What is frequency?

A

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

35
Q

What makes amplitude different from wavelength?

A

amplitude changes the brightness

36
Q

What is spectra?

A

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

37
Q

What is emission spectra?

A

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

38
Q

what are the two types of emission spectra?

A

continuous, line

39
Q

What is an orbital?

A

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

40
Q

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

A

higher; larger; higher

41
Q

What are the four different shapes or orbital subshells?

A

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

42
Q

What is paramagnetism?

A

when some atoms and ions will align (weak magnetism)

43
Q

What is ferromagnetism?

A

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

44
Q

How are ionic bonds classified?

A

a transfer of electrons of metals and nonmetals, 1.7+

45
Q

How are covalent bonds classified?

A

the sharing of electrons between nonmetals

46
Q

How are metallic bonds classified?

A

the pooling of electrons between metals

47
Q

What are valence electrons?

A

electrons in the outermost shell; shared in covalent compounds

48
Q

What ions are the easiest to remove?

A

valence electrons

49
Q

What is polarity?

A

unequal sharing of electrons

50
Q

What is electronegativity?

A

ability of an atom to attract electrons

51
Q

What is a resonance structure in chemistry?

A

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

52
Q

What is the Heisenberg Uncertainty Principle?

A

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

53
Q

What is the Pauli Exclusion Principle?

A

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

54
Q

What is Hund’s rule?

A

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.

55
Q

What is the octet rule?

A

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

56
Q

What is formal charge?

A

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

57
Q

the _shorter___ the bond, the ____ the bond

A

stronger

58
Q

what does nonpolar mean?

A

equal sharing of electrons

59
Q

What does polar mean?

A

unequal sharing of electrons

60
Q

What are columbic forces?

A

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

61
Q

What are the types of electron geometry?

A

Linear, Trigonal planar, Tetrahedral, Trigonal bipyromidal, octohedral

62
Q

What are the types of molecular geometry?

A

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

63
Q
A

Chem 1201 (3 decks)

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