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MCAT Chem > Chem #2 > Flashcards

Chem #2 Flashcards

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1
Q

what are the A elements?

A

representative elements: IA-VIIIA
• Valence electrons in either s or p subshells

this does not have to do with side of the metalloid ladder (just d or p block)

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2
Q

what are the B elements?

A

nonrepresentative elements includes:
• The Transition elements: valence electrons in s and d subshells (these are the elements in the d block)
• And the Lanthanide and actinide series: valence electrons in s and f subshells

this does not have to do with side of the metalloid ladder (just d or p block)

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3
Q

metals

A

left side and middle of the periodic table
o Active metals, transition metals, and lanthanide and actinide series
o Lustrous: shiny solids (except mercury which is a liquid under standard conditions)
o Malleability: ability to be hammered into shapes
o Ductility: pulled or drawn into wires
o Atomic level:
 Low EN (high electropositivity)
 Low effective nuclear charge
o Transition metals have two or more oxidation states (charges when forming bonds with other atoms)
o Conductors: due to valence electrons only being loosely held, they are free to move.
o Want to give up electrons.

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4
Q

what type of elements are lustrous, malleable, ductile, and good conductors?

A

metals

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5
Q

nonmetals

A

found predominately on the upper right side of the periodic table
o Brittle in the solid state with little or no metallic luster
o High IE, EA, and EN
o Poor conductors of heat and electricity
o Inability to give up electrons

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6
Q

what elements want to give up electrons?

A

metals

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7
Q

what elements want to gain electrons

A

nonmetals

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8
Q

metalloids

A

share characteristics with both
o Stairstep pattern that separates the metals from the nonmetals.
o B, Si, Ge, As, Sb. Te, Po, At

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9
Q

effective nuclear charge

A

a measure of the net positive charge experienced by the outermost (valence) electrons.
• Electrons between the valence e and the nucleus can mitigate the pull a little (shielding)

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10
Q

electrons are held _____ tightly further away from the nucleus

A

less

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11
Q

effective nuclear charge does what down a group?

A

stays relatively the same, more positive charge, but pulling on electrons that are in a further shell.

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12
Q

noble/inert gases

A

very stable, Group VIIIA or Group 18

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13
Q

atomic radius

A

o Atomic radius (AR): equal to ½ the distance between the centers of two atoms of an element that are briefly in contact with each other (size of a neutral element)
 As you move left to right, more protons and neutrons being added, greater pull on the electrons that are being added to the same principal energy level, decreases AR
 Move down, valence electrons are put into shells that are further away from the nucleus (greater energy levels), less pull, increase AR

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14
Q

ionic radii

A

 Metals: lose electrons and become positive
• Will have smaller AR
 Nonmetals: gain electrons and become negative
• Will have larger AR
 Metalloids: depends on which side of metalloid line they fall.
 NOTE: elements that are further from the ideal configuration will have more drastic changes to their AR (have to add or lose more electrons to reach this configuration)

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15
Q

what happens to atomic radius as you move left to right and top to bottom?

A

left to right: decrease

top to bottom: increase

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16
Q

cations have ____ atomic radius while anions have _____

A

smaller

larger

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17
Q

ionization energy

A

the energy required to remove an electron from a gaseous species.
o Endothermic process: requires input of heat
o Increases the closer valence electrons are held to the nucleus.
o Subsequent removal of electrons (IE2, IE3) requires even more energy.
o First ionization energy: energy necessary to remove the first electron
o Second ionization energy: energy to remove the second electron
o Active metals: elements in groups IA and IIA, such low ionization energies.

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18
Q

if the ionization energy is huge, probably means the element was in a ____

A

noble gas state

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19
Q

is the second ionization energy always greater than the first?

A

yes

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20
Q

is ionization energy an exothermic or endothermic process?

A

endothermic

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21
Q

ionization energy ______ up and to the right of the periodic table

A

increases

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22
Q

electron affinity

A

the energy dissipated by a gaseous species when it gains an electron.
o Exothermic: process expels energy in the form of heat.
 AE is recorded as a positive number, heat released, but the ΔHrxn is negative.
o The stronger the electrostatic pull (greater the Zeff), the greater the energy release will be when the atom gains the electron.
o Noble gases have close to 0 electron affinity.

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23
Q

electron affinity is endothermic or exothermic

electron affinity is expressed as a ____ number

A

exothermic

positive

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24
Q

electron affinity ____ up and to the right

A

increases

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25
Q

The stronger the electrostatic pull (greater the Zeff), the ____ the energy release will be when the atom gains the electron.

A

greater

26
Q

electronegativity

A

a measure of the attractive force that an atom will exert on an electron in a chemical bond. The greater the EN of an atom, the greater it attracts electrons within a bond.
o Higher EN, higher IE.
o Pauling electronegativity scale: scale used to express EN

27
Q

electronegativity ____ up and to the right of the periodic table

A

up and to the right

28
Q

alkali metals

A

(Group 1): possess most of the classical physical properties of metals, except that their densities are lower than those of other metals
o One loosely bound e- in outermost shell
o Low IE, low EN, low EA, large AR.

29
Q

alkaline earth metals

A

share characteristics with alkali metals, but slightly higher Zeff, so smaller AR.
o Possess 2 loosely bound e- in outermost valence shell.

30
Q

chalcogens

A

(VIA): oxygen group: nonmetals and metalloids
o Crucial for biological functions
o 6 e- in their valence shells
o Elements toward the bottom of the periodic table in this group are toxic

31
Q

halogens

A

• Halogens (VIIA): Cl group: highly reactive nonmetals
o 7 valence electrons
o REALLY want one more e- to fill octet, very reactive
o At standard conditions, can be gaseous (F2 and Cl2) to liquid (Br2) to solid (I2).
o Halides: halogens as ion (normal)
o High EN and EA.

32
Q

noble gases, inert gases

A

filled valence shell so minimal reactivity
o High IE, low EA, He, Ne and Ar have no EN
o Extremely low boiling points and exist as gasses at RT.

33
Q

transition metals

A

(B, groups 3-12): metals
o Low EA, low IE, low EN
o Hard, high melting and boiling points.
o Malleable and good conductors
o Key characteristic:
 Multiple possible oxidation states: represents the number of electrons that an atom can gain, lose, or share when chemically bonding with an atom of another element.
• Due to losing different # electrons from the s- and d- orbitals in their valence shells.
• Many ionic compounds
• Different color based on oxidation state
• Act as cofactors for enzymes
 Complex ions:
• With water: CuSO4 x 5H20 or with nonmetals: Co(NH3)6Cl3
• Formation of complexes splits the d orbitals into 2
 Leads to different solubility
o Complementary color: we observe the color that is not absorbed, the complementary of the color that was absorbed.
 Subtraction frequencies: this color minus this color makes us interpret one color.
• A useful means of predicting the ultimate color appearance of an object if the color of the incident light and the pigments are known.

34
Q

the electron affinity for a noble gas is ___

A

0

35
Q

oxidation state

A

represents the number of electrons that an atom can gain, lose, or share when chemically bonding with an atom of another element.

36
Q

complementary color

A

we observe the color that is not absorbed, the complementary of the color that was absorbed.

37
Q

periodic law

A

the chemical and physical properties of elements are dependent, in a periodic way, upon their atomic numbers

38
Q

which metal is a liquid under standard conditions?

A

mercury

39
Q

______ (metals or nonmetals) have high melting points

A

metals

40
Q

which metal has a very low density

A

lithium

41
Q

malleability

A

the ability of metal to be hammered into shapes

42
Q

ductility

A

the ability of metal to be pulled or drawn into wires

43
Q

electropositivity

A

Electropositivity is the measure of the ability of elements (mainly metals) to donate electrons to form positive ions.

44
Q

removing an electron from an atom requires an input of _____ so it is an _______ process

A

heat

endothermic

45
Q

active metals

A

Groups 1 and 2 because they are so ready to lose an electron or two to obtain the stable octet.

46
Q

the first ionization energy is always _____ than the second ionization energy

A

smaller

47
Q

what is the name of a common scale used to describe electronegativity values?

A

Pauling electronegativity scale

48
Q

For electronegativity, H goes in between the elements ___ and _____

A

B and C

49
Q

The electronegativity value of Neon is very ______

A

low

50
Q

which chemical group reacts violently with water and air

A

alkali metals

51
Q

halogen phases: at standard conditions, F2 and Cl2 are _____, Br2 is ____, and I2 is _____

A

gaseous
liquid
solid

52
Q

noble gases EN, AR, and IE

A

very high IE, close to 0 EA, and first 3 noble gases have negligible EN because they do not typically form bonds

53
Q

noble gases are also known as _____

A

inert gases

54
Q

what is one unique property about transition metals?

A

they can have different oxidations states which makes them very useful in certain biological systems

55
Q

transition metals have the ability to form ____ which causes the ____ to split into two energy sublevels and absorb ____

A

complexes
d orbitals
certain frequencies of light

56
Q

draw the color wheel

A

red orange yellow green blue purple

57
Q

second ionization energy is always ____ than the first ionization energy for an element

A

greater

58
Q

does the number of valence electrons influence the atomic radius of an element?

A

yes, moving to the right in the periodic table adds valence electrons and thus influences effective nuclear charge and atomic radius

59
Q

are alkali metals or alkaline earth metals better conductors?

A

alkali metals

60
Q

Effective nuclear charge: can look at # of protons and # of neutrons and see the ratio

A

ss

61
Q

What is the principal quantum number of the 3d subshell?

A

3

MCAT Chem (12 decks)

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