Ionic Compounds/Polyatomic Compounds (Naming system)

Question 1

is the nonmetal or the metal the cation?

Answer 1

metal

Question 2

is the nonmetal or the metal the anion?

Answer 2

nonmetal

Question 3

True or False: Do the elements in ionic compounds have to not cancel out?

Answer 3

False, it needs to cancel out

Question 4

True or false: Does the cation in an ionic compound ALWAYS come first? And does the anion ALWAYS stay at the end?

Answer 4

yes, yes

Question 5

Ionic Nomenclature Rules

Answer 5

1. Keep the name of the Cation (it will stay the same)
2. Add the -ide suffix to the anion of the compound
   (cut off the end of the elements name to add -ide)

Question 6

Roman Numeral Rules

Answer 6

1. Transition metals can have multiple charges depending on the ion produced
2. Determine the charge and add it after the name of the cation.
3. Will write that charge in roman numerals between the parenthesis
4. You can determine the charge of the cation by knowing the charge of the anion and vice versa
5. Since the molecules have to make a neutral charge, they must all ADD up to 0
6. the anion will have -ide at the end

Question 7

Latin Naming System

Answer 7

1. Find out if the ions in the compound is lesser or greater one (like if an element can be both +2 or +4, find out which one it is)
2. After finding it out, add -ic –> higher charge and -ous –> ous
   *usually applies when the ion is a cation(metal)
3. Add -ide to the anion

Question 8

Can the Latin and Roman Numeral Naming System be used together?

Answer 8

yes

Question 9

What are polyatomic ions

Answer 9

Covalently bonded elements that form a single unit that acts as the anion in the ionic compound

Question 10

Polyatomic Rules for Naming

Answer 10

1. You take the name of the cation
2. And you add the polyatomic ion name
   - Nothing else happens to it

Question 11

What is the naming system for the Halogens in Polyatomic ions?

Answer 11

1 oxygen = add hypo- (at the beginning) and -ite (at the end)
2 oxygens = add -ite
3 oxygens = add -ate
4 oxygens = add per-(at the beginning) and -ate (at the end)

Question 12

Octect Rule

Answer 12

form bonds to have 8 electrons around them (have 2 in each side)

Question 13

Do compounds have one metal and one nonmetal or two nonmetals?

Answer 13

two nonmetals

Question 14

Defining Molecular Compound

Answer 14

• A molecular compound is made up of covalent bonds which involves the sharing of electrons
• Covalent bonds are usually between 2 nonmetals

Question 15

Compounds Nomenclature Rules

Answer 15

1. Use the -ide suffix on the second element (ALWAYS)
2. If there’s only 1 element of the 1st atom, you DONT need the mono prefix
3. If the element starts with AND the prefix ends with “a” or “o”, you will usually drop the last vowel of the prefix

Question 16

name the prefixes for the covalently bonded compounds

Answer 16

mono -1
di - 2
tri - 3
tetra - 4
penta - 5
hexa - 6
hepta - 7
octa - 8
nona - 9
deca - 10

Question 17

Defining Acids

Answer 17

Dissociate in water to produce H+ ions and some anions.

Question 18

Equation that makes up: Binary Acids

Answer 18

Hydrogen + a Halogen

Question 19

Equation that makes up: Oxyacids

Answer 19

Hydrogen + Polyatomic anion

Question 20

Naming System for Binary Acids

Answer 20

1. Acids are named by their ANION (so ignore the H)
2. An element (anion) with the “ide” suffix will change to “ic” and have the prefix “hydro-”
3. Then add the word “acid” after you’re done.

Question 21

Naming System for Oxyacids

Answer 21

1. A polyatomic with the “-ate” suffix will change to “ic”. add the word “acid” after you’re done
2. A polyatomic with the “-ite” suffix will change to “-ous”. add the word “acid” after you’re done
3. Then add the word “acid” after your done

Question 22

What are covant bonds

Answer 22

some valence electrons shared between atoms

Question 23

what are ionic compounds

Answer 23

complete transfer of 1 or more electrons from
one atom to another (one loses, the other gains)
forming oppositely charged ions that attract one
another

Question 24

How to know the electron negativity difference?

Answer 24

if the difference is:
* greater than or equal to 1.9 : ionic
* greater than or equal to 0.5, but less than 1.9 : Polar covalent
* less than 0.5: Non-polar covalent

Question 25

# Bond Polarity 1. A bond is polar if... 2. What are the 2 common exceptions

Answer 25

1. the 2 atoms involved are not the same 2. C-H, and Cl-N bonds

Question 26

# True or False: A molecule that contains polar bonds may or may not be polar, depending on its shape

Answer 26

True

Question 27

# Polar bonds What makes molecules with nonpolar bonds a polar molecule?

Answer 27

if the central atom has one or more lone pairs

Question 28

# Polar bonds What do you need to ask for if a molecule is polar if its bonds are polar?

Answer 28

1. do the inidivudal bond polarities cancel them out? 2. if so, the molecule is nonpolar. If not, then its polar

Question 29

What is a general rule for finding if a molecule is polar or not?

Answer 29

symmetric = nonpolar unsymmetric = polar

Question 30

# molecules w/ 3 atoms * ____ bonds oppose (linear) * ____ bonds oppose (linear) * ____ bonds do not oppose (bent) | 1.

Answer 30

1. equal --> linear (x1 - x2 - x1) 2. unequal --> linear (x1 - x2 - x3) 3. equal --> bent ( x1 - x2 - x1) | the x mean the same or different molecules

Question 31

# Molecules with 4 atoms * ____ bonds oppose in ____ planar arrangment * ____ bonds in ____ planar arrangment | are these nonpolar or polar

Answer 31

1. equal, trigonal --> nonpolar 2. unequal, trigonal --> polar

Question 32

# Molecular Shapes How can we predict the 3D structure of a moleucles just by ...

Answer 32

ading up: bonded atoms + lone pairs

Question 33

# What determins the Shape of a molecule? - True or False? Do bonded atoms and lone pairs take up less space and prefer to be closer to each other as possible

Answer 33

FALSE; bonded atoms and lone pairs take up space and prefer to be as far from each other as possible

Question 34

# True or False: does a central atom have 4 "things" around it? And what are those "things"

Answer 34

Yes it does. Things - is an atom or a lone pair of electrons

Question 35

how do you find the # of "things" in a molecule?

Answer 35

atoms + lone pairs

Question 36

# Geometries What is the: 1. # of things 2. geometry 3. bond angles of linear

Answer 36

1. 2 things 2. linear 3. 180 degrees

Question 37

# geometries What is the: 1. # of things 2. geometry 3. bond angles of trigonal planar

Answer 37

1. 3 things 2. trigonal planar 3.120 degrees

Question 38

# geometries What is the: 1. # of things 2. geometry 3. bond angles of tetrahedral

Answer 38

1. 4 things 2. tetrahedral 3. 109.5

Question 39

# geometries What is the: 1. # of things 2. geometry 3. bond angles of trigonal bipyrimidal

Answer 39

1. 5 things 2. trigonal bipryimidal 3. 120 and 90 degrees

Question 40

# geometries What is the: 1. # of things 2. geometry 3. bond angles of octahedral

Answer 40

1. 6 2. octrahedral 3. 90 degrees

Question 41

# molecular geometries what is the "shape" of the molecule defined by? ## Footnote the geometry is often NOT the shape of the molecule

Answer 41

the positions of only the atoms in the molecules, not the lone pairs

Question 42

# Geometry vs. Shape Within each (electron doman) geometry, there might be more than one ____

Answer 42

shape (molecular geometry)

Question 43

# Linear geometry: 2 things - true/false in this geometry, there is only 1 molecule geometry: linear Note: if there are only 2 atoms in the molecules, the molecules won't be linear no matter what the geometry is

Answer 43

Part 1: True Part 2: False - If there are only two atoms in the molecule, the molecule will be linear no matter what the geometry is.

Question 44

# Trigonal Planar geometry: 3 things 2 molecule geometries:

Answer 44

* Trigonal planar, if there are no lone pairs * Bent, if there is a lone pair

Question 45

# Lone pairs and Bond Angle Are lone pairs physically smaller or larger than atoms? And is their repulsion smaller or larger? What happens to the bond in the angle of the molecule then?

Answer 45

* Lone pairs are physically larger than atoms. * Therefore, their repulsions are greater; this tends to decrease bond angles in a molecule.

Question 46

# Tetrahedral geometry: 4 things * There are three molecular geometries:

Answer 46

* Tetrahedral, if no lone pairs * Trigonal pyramidal if one is a lone pair * Bent if there are two lone pairs

Question 47

# Trigonal Bipyramidal: geometry 5 things * There are two distinct positions in this geometry:

Answer 47

* Axial * Equatorial

Question 48

# Trigonal Bipyramidal geometry There are four distinct molecular geometries in this domain:

Answer 48

* Trigonal bipyramidal (lp - 0) * Seesaw (lp - 1) * T-shaped (lp - 2) * Linear (lp - 3)

Question 49

# Octahedral geometry 6 things 3 molecular geometries:

Answer 49

* octahredral (lp - 0) * square pyramidal (lp - 1) * square planar (lp - 2) | lp = lone pair(s)

Question 50

# Hydrates Naming System Some compound shave water molecules attaches as part of their strucuture - called hydrates So, whats the naming system? | ex - CuSO4 5H2O copper(II)sulfate pentahydrate

Answer 50

1. add the cation name (put the roman numberal if transition metal) 2. Add the polyatomic anion name 3. the number of H20 molecules will have greek prefixes in front of the word **hydrate**

Question 51

# periodic trends Atomic Radius

Answer 51

The distance between an atom’s nucleus and its valence electrons * Across a period - smaller * down a group - larger