Chapters 4-6 (Exam 2)

Question 1

How is the periodic table ordered?

Answer 1

In increasing atomic number values

Question 2

What is a many electron system?

Answer 2

Atoms with more than one electron

Question 3

What does the Pauli exclusion principle state

Answer 3

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./

Question 4

What is the Aufban princible

Answer 4

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

Question 5

What is Hund’s rule

Answer 5

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

Question 6

What are paired electrons called?

Answer 6

Diamagnetic

Question 7

What are unpaired electrons called?

Answer 7

Paramagnetic

Question 8

Diamagnetic substances are ______ by magnetic fields

Answer 8

Repelled

Question 9

Paramagnetic substances are _____ by magnetic fields

Answer 9

Attractred

Question 10

What are the core electrons

Answer 10

The electrons that make up the noble gas core

Question 11

What are the valence electrons

Answer 11

The electrons in the outermost occupied shell

Question 12

What is Nuclear charge (and its symbol)

Answer 12

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

Question 13

What is Effective Nuclear Charge

Answer 13

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

Question 14

Effective nuclear charge formula

Answer 14

Zeff = Z - o

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

Question 15

What is metallic radius

Answer 15

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

Question 16

What is covalent radius

Answer 16

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

Question 17

What is Ionization energy

Answer 17

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

Question 18

What is a cation and when does it appear

Answer 18

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

Question 19

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

Answer 19

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

Question 20

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

Answer 20

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

Question 21

What is electron affinity

Answer 21

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

Question 22

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

Answer 22

349.0 kJ/mol

Question 23

What is an anion

Answer 23

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

Question 24

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

Answer 24

decreases, increases, largest is bottom left

Question 25

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

Answer 25

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

Question 26

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

Answer 26

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

Question 27

Metals tend to:

Answer 27

- be shiny and malleable and ductile - be good conductors of heat and electricity - Have low ionization energies (commonly form cations)

Question 28

Nonmetals tend to:

Answer 28

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

Question 29

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

Answer 29

decreases, increases

Question 30

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

Answer 30

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

Question 31

What is the formula for Coulomb's law?

Answer 31

F = (Q1 x Q2) / d^2

Question 32

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

Answer 32

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

Question 33

What is an isoelectronic series

Answer 33

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

Question 34

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

Answer 34

largest

Question 35

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

Answer 35

smallest

Question 36

What are degenerate electrons

Answer 36

Electrons that match each others energy

Question 37

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

Answer 37

increases, decreases, highest is top right

Question 38

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

Answer 38

Increases, decreases, highest top right

Question 39

Ionization ____ an electron and Electron affinity ____ an electron

Answer 39

removes, adds

Question 40

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

Answer 40

mixtures, but not compounds

Question 41

What types of elements form an ionic compound?

Answer 41

cations and anions

Question 42

What is a binary compound?

Answer 42

An ionic compound consisting of one metal and one non metal

Question 43

What is the ion of Na.

Answer 43

Na^+ + e^-

Question 44

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

Answer 44

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

Question 45

What does ionization do and what does it look like?

Answer 45

it removes an electron and is represented by a plus sign

Question 46

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

Answer 46

it adds an electron and is represented by a minus sign

Question 47

What is Lattice energy

Answer 47

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.

Question 48

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

Answer 48

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

Question 49

With ions with different charges, use _____

Answer 49

Roman numerals

Question 50

How do you name an anion (negative charge)

Answer 50

add "-ide ion" to the end | ex: chloride

Question 51

How do you figure out how much

Answer 51

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

Question 52

correct wording for FeCl2

Answer 52

Iron (II) Chloride

Question 53

What is a covalent bond

Answer 53

when electrons are shared

Question 54

What is a molecule?

Answer 54

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

Question 55

What are molecules containing more than two atoms referred to

Answer 55

Polyatomic molecules

Question 56

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

Answer 56

homonuclear diatomic molecule

Question 57

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

Answer 57

hetero diatomic molecule

Question 58

What is a molecular formula

Answer 58

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

Question 59

What is an allotrope

Answer 59

one of two ore more distinct forms of an element | - Ex: O2 and O3

Question 60

What a structural formula

Answer 60

A visual representation of the general arrangement of atoms

Question 61

What is the empirical formula

Answer 61

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

Question 62

Greek prefixes for numbers | 1, 2, 3, 4, 5, 6, 7, 8, 9, 10

Answer 62

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

Question 63

When naming mixtures, would it be pentoxide or pentaoxide

Answer 63

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

Question 64

Hydrogen compounds: What is the name of B2H6

Answer 64

Diborane

Question 65

Hydrogen compounds: What is the name of SiH4

Answer 65

Silane

Question 66

Hydrogen compounds: What is the name of NH3

Answer 66

Ammonia

Question 67

Hydrogen compounds: What is the name of PH3

Answer 67

Phosphine

Question 68

Hydrogen compounds: What is the name of H2O

Answer 68

Water

Question 69

Hydrogen compounds: What is the name of H2S

Answer 69

Hydrogen Sulfide

Question 70

What is an acid

Answer 70

A substance that produces hydrogen ions when dissolved in water

Question 71

What is the formula for naming acids

Answer 71

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

Question 72

What is an inorganic compound

Answer 72

compounds that do not have carbon

Question 73

What is an organic compound

Answer 73

compounds that have carbon and hydrogen, and sometimes other elements

Question 74

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

Answer 74

Hydrocarbons

Question 75

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

Answer 75

You take out the hydro. | - Ex: H2SO4 is Sulfuric acid

Question 76

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

Answer 76

Hydroxide at the end

Question 77

What is a hydrate compound

Answer 77

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

Question 78

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

Answer 78

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

Question 79

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

Answer 79

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

Question 80

What is 1 amu

Answer 80

1.661 x 10^-24 g

Question 81

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

Answer 81

Mass - Moles - Particles Divide when going in, multiply when going out

Question 82

How do you find the empirical formula from the molecular formula

Answer 82

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

Question 83

What are Polyatomic molecules

Answer 83

molecules containing more than two atoms referred to

Question 84

What is a homonuclear diatomic molecule

Answer 84

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

Question 85

What is the octet rule?

Answer 85

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

Question 86

What are leftover electrons called in Lewis structure

Answer 86

lone pairs

Question 87

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

Answer 87

stronger