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Chem 101 > Chapters 4-6 (Exam 2) > Flashcards

Chapters 4-6 (Exam 2) Flashcards

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1
Q

How is the periodic table ordered?

A

In increasing atomic number values

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2
Q

What is a many electron system?

A

Atoms with more than one electron

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3
Q

What does the Pauli exclusion principle state

A

No two eletrons in an atom in the gorund state can have the same four quantum numbers; If they have the same n, l, and ml values, the ml, or spin, must be differetn./

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4
Q

What is the Aufban princible

A

building the periodic table of elemtnets and determining their electron configurations by steps.

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5
Q

What is Hund’s rule

A

The most stable arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with the same spin is maximized

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6
Q

What are paired electrons called?

A

Diamagnetic

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7
Q

What are unpaired electrons called?

A

Paramagnetic

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8
Q

Diamagnetic substances are ______ by magnetic fields

A

Repelled

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9
Q

Paramagnetic substances are _____ by magnetic fields

A

Attractred

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10
Q

What are the core electrons

A

The electrons that make up the noble gas core

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11
Q

What are the valence electrons

A

The electrons in the outermost occupied shell

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12
Q

What is Nuclear charge (and its symbol)

A

(Z)It is the number of protons in the nucleus of an atom

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13
Q

What is Effective Nuclear Charge

A

(Zeff) the actual magnitude of positive charge that is “experienced” by an electron in the atom.

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14
Q

Effective nuclear charge formula

A

Zeff = Z - o

where o is the shielding constant, greater than zero but smaller than Z.

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15
Q

What is metallic radius

A

Half the distance between the nuclei of two adjaent, identical metal atoms.

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16
Q

What is covalent radius

A

Half the distance between adjacent, identical nuclei that are connected by a chemical bond

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17
Q

What is Ionization energy

A

the minimum energy required to remove an electron from an atom in the gas phase

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18
Q

What is a cation and when does it appear

A

an ion with a net positive charge, it appears when an electron is lost

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19
Q

What is easier to remove, an electron in an s orbital or one in a p orbital

A

The p orbital is easier to remove, and the s orbital is harder to remove

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20
Q

What’s easier to remove, an electron in a singly-occupied orbital, or an electron in a doubly occupied orbital.

A

An electron in a doubly occupied orbital is easier to remove, and an electron in a singly occupied orbital is harder to remove

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21
Q

What is electron affinity

A

Energy released when an atom in the gas phase accepts an electron

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22
Q

How much energy is accepted when a mole of gaseous chlorine atom accepts a mole of electrons

A

349.0 kJ/mol

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23
Q

What is an anion

A

An ion whose net charge is negative due to an increase in the number of electrons

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24
Q

Atomic radius ______ from left to right, and _______ from up to down

A

decreases, increases, largest is bottom left

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25
Q

Whats easier to add, an electron to an s orbital or an electron to a p ortbital

A

It is easier to add a electron to an s orbital, and harder to add an electron to a p orbital

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26
Q

Whats easier to add, an electron to a empty occupied orbital, or an electron to a single occupied orbital

A

It is easier to add an electron to an empty orbital, and it is harder to add an electron to a singurly occupied orbital.

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27
Q

Metals tend to:

A
  • be shiny and malleable and ductile
  • be good conductors of heat and electricity
  • Have low ionization energies (commonly form cations)
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28
Q

Nonmetals tend to:

A
  • vary in color and lack shininess
  • Be brittle
  • Be poor conductors of heat or electricity
  • Have high electron affinities (commonly form anions)
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29
Q

Metallic characteristics _____ from left to right and _______ from top to bottom

A

decreases, increases

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30
Q

Why do some elements share properties with the elements located down and to the right diagonal to them?

A

The charge of the densities of their cations are comparable, which would mean they have similar properties.

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31
Q

What is the formula for Coulomb’s law?

A

F = (Q1 x Q2) / d^2

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32
Q

How can you find out the number of anions in a some groups

A

Most of the anions that form from elements in Groups 14-17 have charges equal to their groups last digit minus 8

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33
Q

What is an isoelectronic series

A

A series of two or more species that have identical electron configurations, but different nuclear charges.

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34
Q

In an isoelectronic series, the species with the smallest nuclear change (smallest atomic number, Z) will have the ______ radius

A

largest

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35
Q

In an isoelectronic series, the species with the largest nuclear change (largest atomic number, Z) will have the ______ radius

A

smallest

36
Q

What are degenerate electrons

A

Electrons that match each others energy

37
Q

Electron affinity ______ from left to right and _______ from top to bottom

A

increases, decreases, highest is top right

38
Q

Ionization energy ______ from left to right and _______ from top to bottom

A

Increases, decreases, highest top right

39
Q

Ionization ____ an electron and Electron affinity ____ an electron

A

removes, adds

40
Q

which can be separated into similar substances by a physical process?

A

mixtures, but not compounds

41
Q

What types of elements form an ionic compound?

A

cations and anions

42
Q

What is a binary compound?

A

An ionic compound consisting of one metal and one non metal

43
Q

What is the ion of Na.

A

Na^+ + e^-

44
Q

What is the structure of an ion compouned called and look like

A

lattice and it is a three dimensional network of alternation cations and anions

45
Q

What does ionization do and what does it look like?

A

it removes an electron and is represented by a plus sign

46
Q

What does electron affinity do and what does it look like?

A

it adds an electron and is represented by a minus sign

47
Q

What is Lattice energy

A

the amount of energy needed to convert a mole of ionic solid to its ions in the gas phase, it is a measure of how stable the ionic compound is.

48
Q

How do you name a cation (positive charge) and what is K and K+

A

You add ion to the end. One is potassium and the other is a potassium ion

49
Q

With ions with different charges, use _____

A

Roman numerals

50
Q

How do you name an anion (negative charge)

A

add “-ide ion” to the end

ex: chloride

51
Q

How do you figure out how much

A

you take the value of the charge and use it for the amount of the other element

52
Q

correct wording for FeCl2

A

Iron (II) Chloride

53
Q

What is a covalent bond

A

when electrons are shared

54
Q

What is a molecule?

A

A neutral combination of at least two atoms in a specific arrangement held together by bonds

55
Q

What are molecules containing more than two atoms referred to

A

Polyatomic molecules

56
Q

What is it called when both atoms are the same in a molecule

A

homonuclear diatomic molecule

57
Q

What is it called when both atoms are different in a molecule

A

hetero diatomic molecule

58
Q

What is a molecular formula

A

a formula that shows the exact number of atoms of each element in a molecule.

59
Q

What is an allotrope

A

one of two ore more distinct forms of an element

- Ex: O2 and O3

60
Q

What a structural formula

A

A visual representation of the general arrangement of atoms

61
Q

What is the empirical formula

A

It tells what elements are present in a molecule and in what whole number ratio they are combined
- EX: molecular formula is H2O2 but the empirical formula is HO

62
Q

Greek prefixes for numbers

1, 2, 3, 4, 5, 6, 7, 8, 9, 10

A 
Mono - 1
Di - 2
Tri - 3
Tetra - 4 
Penta - 5
Hexa - 6
Hepta - 7
Octa - 8
Nona - 9
Deca - 10
63
Q

When naming mixtures, would it be pentoxide or pentaoxide

A

Pentoxide because the -o and -a are usually omitted from the greek prefixes

64
Q

Hydrogen compounds: What is the name of B2H6

A

Diborane

65
Q

Hydrogen compounds: What is the name of SiH4

A

Silane

66
Q

Hydrogen compounds: What is the name of NH3

A

Ammonia

67
Q

Hydrogen compounds: What is the name of PH3

A

Phosphine

68
Q

Hydrogen compounds: What is the name of H2O

A

Water

69
Q

Hydrogen compounds: What is the name of H2S

A

Hydrogen Sulfide

70
Q

What is an acid

A

A substance that produces hydrogen ions when dissolved in water

71
Q

What is the formula for naming acids

A
  1. Change hydrogen to hydro-
  2. take the second element and take out -ide and add -ic
  3. add acid
72
Q

What is an inorganic compound

A

compounds that do not have carbon

73
Q

What is an organic compound

A

compounds that have carbon and hydrogen, and sometimes other elements

74
Q

What are the simplest organic compounds that contain only carbon and hydrogen called?

A

Hydrocarbons

75
Q

What do you do when naming acids and there are 2 elements after the hydrogen

A

You take out the hydro.

- Ex: H2SO4 is Sulfuric acid

76
Q

If there is a OH in the element what do you name it

A

Hydroxide at the end

77
Q

What is a hydrate compound

A

A compound that has a specific number of water molecules in it.

78
Q

How to find the molecular mass, or molecular weight, of a compound

A

You multiply the quantity of an element with the atomic mass of the elements and add it all up, for compounds its called the formula mass or formula weight

79
Q

How do you find the percent compositon of compounds for each element?

A

(n x atomic mass of element) / (formula mass of compound) all times 100%

80
Q

What is 1 amu

A

1.661 x 10^-24 g

81
Q

What is the conversion trick for particles, moles, and mass.

A

Mass - Moles - Particles

Divide when going in, multiply when going out

82
Q

How do you find the empirical formula from the molecular formula

A

You can divide the molar mass of the formula by the empirical formula of the other and figure out the ratio of elements.

83
Q

What are Polyatomic molecules

A

molecules containing more than two atoms referred to

84
Q

What is a homonuclear diatomic molecule

A

What is it called when both atoms are the same in a molecule

85
Q

What is the octet rule?

A

Atoms will lose, gain, or share electrons to achieve a noble gas electron configuration

86
Q

What are leftover electrons called in Lewis structure

A

lone pairs

87
Q

The shorter distance the molecules are together, the _____ the bond

A

stronger

Chem 101 (4 decks)

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