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Chemistry R120 > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

What are periods in the Periodic Table?

A

horizontal (left to right)

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2
Q

What are groups in the Periodic Table?

A

verticle (up and down)

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3
Q

What are valence orbitals?

A

occupied orbitals that hold valence electrons | elements in the same column/group have same #valence electrons

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4
Q

Who is Dmitri Mendeleev?

A

used chemcial properties to organize the table

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5
Q

Who arranged the elements based on weight?

A

Dmitri Mendeleev and Lothar Meyer

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6
Q

Who is Henry Mosely?

A

developed the concept of atomic number after Rutherford’s discovery of the nuclear atom

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7
Q

What is periodicity?

A

repetitive pattern of a property for elements based on atomic number

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8
Q

What is effective nuclear charge?

A

net positive charge experienced by an electron in an atom

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9
Q

What is the effective nuclear charge (Zeff) not the full nuclear charge?

A

the core (inner shell) electrons shield the valence (outer shell) electron from nucleus = valence e- experiences forces from core e- repulsion and nucleus attraction

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10
Q

What is the periodic TREND for effective nuclear charge?

A

increases left–>right | slight increases down a group

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11
Q

What are van der Waals radius?

A

nonbonding radius | half the shortest distance separating 2 nuclei during a collision between atoms

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12
Q

what is a bonding atomic radius?

A

half the distance between 2 bonded atoms

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13
Q

What is the periodic TREND for atomic size?

A

increases right –> left (opposite of Zeff) | increases down a group

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14
Q

What are ionic radii?

A

determined by the interatomic distances in ionic compounds

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15
Q

What are the 3 things ionic size depends on?

A

nuclear charge | #electrons | orbitals in which electrons are in

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16
Q

What is the size of cations compared to their parent atom?

A

SMALLER than parent atom

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17
Q

What is the size of anions compared to their parent atom?

A

LARGER than parent atom (more electrons = increase repulsion = bigger e- cloud)

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18
Q

What is the isoelectric series?

A

ions have the same number of electrons

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19
Q

What are the 5 ions that all have 10 electrons?

A

O2- | F- | Na+ | Mg2+ | Al3+

20
Q

What is ionizing energy?

A

minimum energy required to remove an electron of a gaseous atom/ion from ground state

21
Q

What is the first ionization energy?

A

to remove the 1st electron

22
Q

What is the second ionization energy?

A

to remove the 2nd electron

23
Q

What is the relationship between removing an electron and the ionization energy?

A

higher ionization energy = more difficult to remove electron

24
Q

What is the periodic TREND for the 1st ionization energy (I1)?

A

increases left –>right | increases up a group | s/p > d > f

25
Q

What are the 3 factors that affect ionization energy?

A

atomic size (smaller = higher I) | Zeff | avg. nucleus -electron distance

26
Q

What are the 2 situations when the trend for ionization energy doesn’t apply?

A

when the added valence e- in the next element: enters a new higher energy state | is first e- pair in one box (orbital) of a sublevel (degenerate orbitals)

27
Q

What is the electron configuration for cations?

A

lost from the highest energy level (n)

28
Q

What is the electron configuration for anions?

A

filled up to ns2 np6

29
Q

What is electron affinity?

A

energy change accompanying the electron addition to a gas atom

30
Q

What is the difference between ionization energy and electron affinity?

A

both measure energy change: | IE = when atom LOSES an electron ; EA = when atom GAINS an electron

31
Q

What is the general period TREND for electron affinity?

A

increases left –> right

32
Q

What are the 3 exceptions to the periodic trend for electron affinity?

A

Group 2A = s-orbital full = X- unstable = decrease EA | Group 8A = p-orbital full = X- unstable = decrease EA | Group 5A = p-orbital partially full = can add e- = slight decrease EA

33
Q

What are the 7 properties of metals?

A

abundant in nature | form cations | shiny luster | conduct heat/electricity | malleable/ductile | solids @RT (not Hg) | low IE

34
Q

What are the 2 properties of metals in chemical reactions?

A

metal oxides = basic | metal+nonmetal = ionic compound

35
Q

What are the 6 properties of nonmetals?

A

Right side of table | form anions | dull/brittle solids | can be in any form (g, l, s) | large negative electronegativity | poor conductors

36
Q

What are the 2 properties of nonmentals in chemical reactions?

A

nonmetal oxides = acidic | nonmetal+nonmetal = molecular compound

37
Q

What are metalloids?

A

have a mix characteristics of some metal and nonmetal properties

38
Q

What is a characteristic of metalloids?

A

electrical semi-conductors

39
Q

What are the 6 metalloids?

A

B, Si, Ge, As, Sb, Te

40
Q

What is the Group 1A metals called?

A

alkali metals

41
Q

What are the 6 characteristics/properties of alkali metals?

A

soft/metallic solids | only found as compounds in nature | metallic properties | LOW melting points/densities | low IE | exothermic when react with H2O

42
Q

What are the Group 2A metals called?

A

alkaline earth metals

43
Q

What are the 3 characteristics of alkaline earth metals?

A

higher melting points/densities than Group 1A | slightly higher IE than Group 1A | increase reactivity down the group

44
Q

What is the periodic TREND for Group 6A?

A

increase metallic character down the group

45
Q

What is the periodic TREND for Group 7A

A

high EA all around

46
Q

What is Group 7A called? What is its characteristic?

A

halogens | reacts readily with metals = halides

47
Q

What is Group 8A called? What are its 4 characteristics?

A

noble gases | highest EA | unreactive | found as monoatomic gases | LARGE IE

Chemistry R120 (18 decks)

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