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Chemistry 11 > Chapter 6: Relationships and Patterns in Chemistry > Flashcards

Chapter 6: Relationships and Patterns in Chemistry Flashcards

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1
Q

who came up with the idea of conservation of mass?

A

Antoine Laurent de Lavoisier

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2
Q

who said this: “Nothing is lost, nothing is created, everything is transformed”

A

Antoine Laurent de Lavoisier

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3
Q

Johann Döbereiner realized he could organize certain elements into groups of _____ which he called ______

A

three called triads

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4
Q

Antoine Émile Béguyer de Chancourtois was the first to recognize the ________ of elements

A

periodicity

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5
Q

in what order did Chancourtois organize the elements?

A

by atomic weight

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6
Q

Julius Lothar Meyer published the periodic table based on the _______ of each element?

A

valency

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7
Q

John Newlands noticed that some trends were based of off which number? What was the name of this law?

A

8

law of octaves

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8
Q

Dimitry Mendeleev ordered the periodic table by _______?

A

molar mass

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9
Q

T or F: Mendeleev left empty spots in his table?

A

True, he predicted undiscovered elements that would take those places

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10
Q

def: arranging the elements by increasing aotmic mass produced an observable patter in which similar properties repeat on a regular basis, or periodically

A

periodic law

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11
Q

what were two problems with Mendeleev’s table?

A
  1. it didn’t predict the noble gases (they don’t react so it’s hard to discover them)
  2. it couldn’t locate hydrogen, as it fit in multiple places
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12
Q

who reordered the periodic table based on atomic number?

A

Henry Moseley

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13
Q

what are the elements 93-118 called?

A

the trans-uranium elements

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14
Q

def: horizontal rows on the periodic table, where atomic number increases by one and properties gradually change from one end to the other

A

periods

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15
Q

def: vertical columns on the periodic table, in which elements have similar properties, owing to the similarity of their electron configurations

A

groups (families)

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16
Q

def: groups 1 & 2 (s block) and 13-18 (p-block) on the periodic table, except hydrogen

A

main group elements

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17
Q

def: groups 3-12 on the periodic table, encompassing all the metals of the d and f blocks

A

transition metals

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18
Q

def: two rows of elements generally placed below the main table, comprising the metals of the f block

A

inner transition metals

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19
Q

def: elements Z = 57 through Z = 71, lanthanum through lutetium

A

lanthanides

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20
Q

def: elements Z = 89 through Z = 103, actinium through lawrencium

A

actinides

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21
Q

def: any of an atom’s electrons that can participate in bond formation with other atoms, whether ionically or covalently

A

valence electron

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22
Q

for transition metals, valence electrons are all those _______ the ________, regardless of their principal quantum number

A

outside the atom’s noble gas core

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23
Q

def: any of an atom’s electrons that isn’t a valence electron and that doesn’t participate in bond formation

A

core electron

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24
Q

def: the metallic elements of the periodic table that fall between the transition metals and the metalloids

A

post-transition metals

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25
Q

def: predictable and regular patterns of cyclical change in elemental properties throughout the periodic table, moving either vertically or horizontally

A

periodic trends

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26
Q

def: an expression of the size of an atom, representing the typical distance from the centre of it’s nucleus to the boundary of its electron cloud

A

atomic radius

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27
Q

why can’t we determine the precise size of an atom?

A

because the electron cloud does not have distinct boundaries

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28
Q

def: an estimate of the size of an atom, based on half the distance between covalently bonded atoms

A

covalent radius

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29
Q

def: an estimate of the size of a metal atom, based on half the distance between the nuclei and adjacent atoms in a metal lattice

A

metallic radius

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30
Q

what two factors influence the size of an atom’s electron cloud?

A
  • how many energy shells contain electrons

- the amount, nature and separation of charge within the atom

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31
Q

as the principle quantum number goes up, the number of outermost shells _____ and they get _____ in distance to the nucleus

A

goes up and they get further away

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32
Q

what force are neutrons held together by?

A

residual strong force

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33
Q

T or F: adding more electrons and protons increases the amount of opposite charge in the atom, increasing the nucleus’s inward pull on the valence electrons, making atoms smaller across the table

A

True

34
Q

def: the repulsive action of inner core electrons on outer valence electrons, effectively reducing the nucleus’s inward pull, causing the atom to increase in size

A

shielding effect

35
Q

def: the net positive charge experienced by an electron in a multi-electron atom, representing less than the full nuclear charge as inner electrons repel outer electrons, offsetting some of the nucleus’s inward pull

A

effective nuclear charge (Zeff)

36
Q

when metals form cations, what happens to their ionic size?

A

it’s smaller than it’s atomic radius

37
Q

when non-metals form anions, what happens to their ionic size?

A

it’s larger than it’s atomic radius

38
Q

def: the amount of energy required to remove the most loosely held electron from a gaseous atom to form a cation to increase its positive charge

A

ionization energy (IE)

39
Q

generally speaking, each electron is ____ to remove than the last

A

harder

40
Q

as Zeff increases, atoms become ______ and electrons become more ____ to remove, causing an ________ in ionization energy

A

atoms become smaller and electrons become more difficult to remove, causing an increase in ionization energy

41
Q

def: a chemical property that describes an atom’s (or a group of atoms’) ability to attract electrons towards itself

A

electronegativity (EN)

42
Q

def: the change in energy when an atom gains an electron to form an anion, or when an anion gains another electron, increasing its negative charge

A

electron affinity

43
Q

the stronger an element attracts electrons, the _____ energy it releases when gaining an electron, making its electron affinity ______

A

the more energy releases when gaining an electron, making its electron affinity greater

44
Q

def: a numerical value representing the difference in the electronegativities of two atoms

A

ΔEN

45
Q

metals have relatively _____ ionization energies

A

low

46
Q

non-metals have relatively _____ electronegativities

A

high

47
Q

non-metals have relatively _____ electron affinities

A

high

48
Q

an ionic bond will form between a metal and a non metal if their ΔEN is greater than _____

A

1.7

49
Q

a covalent bond will form between two non-metals if their ΔEN value is less than _______

A

1.7

50
Q

def: a covalent bond between non metal atoms with the same electronegativities, where electron sharing is equal

A

non polar covalent bond

51
Q

a non polar covalent bond forms between two non-metals if their ΔEN value between ____ and _____

A

0 and ~ 0.4

52
Q

def: a covalent bond between two non-metals in which electron sharing is sufficiently unequal that the bond displays significant and meaningful ionic nature

A

polar covalent bond

53
Q

def: the non-integer charge values at the ends of a polar covalent bond, due to the uneven distribution of electron density within the bond

A

partial ionic charges

54
Q

def: a simplified diagram that communicates molecular structure using element’s symbol as well as dots and lines

A

Lewis Structure

55
Q

which two noble gases form compounds?

A

xenon and krypton

56
Q

def: describes an atom’s combining power, often in terms of how many hydrogen atoms it can covalently bond with, or how many chloride anions it can ionically bond with

A

valency

57
Q

rather than lattices, covalent compounds form______

A

separate and distinct molecules

58
Q

def: any pair of valence electrons that are nonbonding, as atoms don’t share them with other atoms

A

lone pair

59
Q

T or F: Lone pairs may form or disperse because of bond formation

A

True

60
Q

def: an observational rule in chemistry that says the valence shells of the first-period elements hydrogen and helium can hold a maximum of two electrons, never more

A

duet rule

61
Q

which atoms do not obey or exceed the octet rule?

A

H, He, Be, B, Al

62
Q

def: an observational rule of thumb in chemistry that says main-group elements from periods 2 to 7 seek to have eight electrons in their valence shell

A

octet rule

63
Q

T or F: the central atom in a binary compound is usually the one of lower electronegativity

A

True

64
Q

def: covalent bonding between two atoms who share more than two electrons

A

multiple bonds

65
Q

def: a configuration of elements from periods 3 to 7, in which their valence shells expand past eight electrons as the central atom, as they can incorporate d orbitals

A

expanded octet

66
Q

def: different, but equivalent Lewis structures of the same molecule, showing all the possible double bond locations, connected by a double headed arrow

A

resonance structures

67
Q

def: electrons in a molecule, ion or solid metal that aren’t associated with a single atom or covalent bond, allowing them to be covalent to more than two atoms

A

delocalized electrons

68
Q

electron delocalization allows the creation of an _________

A

electrical current

69
Q

def: a model chemists use to predict a molecule’s geometry based on how many groups of electrons surround the central atom, both bonding electrons and lone pairs

A

valence shell electron pair repulsion theory

VSEPR

70
Q

def: a number used in VSEPR theory to predict molecular geometry, that is equal to the number of peripheral atoms plus the number of lone pairs

A

steric number

71
Q

how do you find the steric number?

A

peripheral atoms + lone pairs = steric number

72
Q

def: the superposition or mixing of atomic orbital wave functions to produce new hybrid orbitals with unique shape and energies

A

orbital hybridization

73
Q

def: the strongest type of covalent bond, formed between two atoms when their orbitals overlap head on

A

sigma bond

74
Q

def: a second type of covalent bond that is weaker than a sigma bond, formed between two atoms when their p orbitals are parallel and overlap side on

A

pi bond

75
Q

def: a vector quantity that expresses a bond’s polarity, showing the separation of opposing charges, and the directionality of that separation (a moment)

A

bond dipole moment

76
Q

T or F: A polar bond has a relatively large ΔEN value, producing a bond dipole moment that is not strong
enough to affect behaviour, while a non-polar bond’s ΔEN value produces one that is

A

False

77
Q

def: a molecule that has an overall, or net dipole moment, because of it’s bond polarities and its molecular geometry

A

polar molecule

78
Q

T or F: Polar molecules must contain polar bonds, but cannot be symmetrical, in both structure and
composition – polar bonds and asymmetrical structure or composition make polar molecules

A

True

79
Q

def: the attractive force that exists between the partial positive charge of one polar molecule and the partial negative charge of another

A

dipole-dipole force

80
Q

def: an electrostatic attraction that forms between the partially positive hydrogen in a highly polarized bond (usually H-N, H-O, and H-F) and the negative lone pair on a nearby atom

A

hydrogen bond

81
Q

def: a weakly attractive force that forms when non polar molecules gain temporary dipole moments

A

London dispersion forces

Chemistry 11 (6 decks)

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