Chemistry (Unit 2)

Front 1

What is a formula unit?

Back 1

The fundamental particle held together by an ionic bond

- could you just call it an ionic compound?????

Front 2

What is a molecule?

Back 2

The fundamental particle held together by a covalent bond.

Front 3

True or False?

Diatomic Molecule are always Polar.

Back 3

False,

Diatomic Molecules are always non-polar because the two atoms have the same electronegativity

Front 4

What is a Polar Bond?

Back 4

A polar bond is one in which one atom in the bond has a stronger attraction than the other atom for the electron pair (and essentially holds them closer)

Front 5

Non-Polar Bond

Back 5

When two atoms in a bond have the same attraction for the electron pair (same electronegaivity)

Front 6

When is Delta Notation used, what does it look like and what does the notation refer to?

Back 6

It is used to show which atom, in a polar bond, has the greater electronegativity.

- It looks like this S(-), S(+) denoted above the formula

- The S refers to slightly. = Slightly more negative OR slightly more positive

Front 7

What atoms form covalent bonds?

Back 7

2 or more non-metals

Front 8

What is a double bond

Back 8

When 2 atoms form a covalent bond by sharing 2 pairs of loose electrons

Front 9

What is a triple bond?

Back 9

When 2 molecules form a covalent bond by sharing three pairs of loose electrons

Front 10

True or False?

A chemical bond containing a metal is always an ionic bond

Back 10

True

Front 11

What is Electronegativity?

Back 11

The measure of the ability of an atom to attract electrons in a chemical bond.

Front 12

What are the elements that naturally form diatomic covalent bond?

Back 12

H, O, F, N, I, Cl, Br

Hint 12

H-appy

O-n

F-riday

N-ight

I-ce

Cl-Cold

Br-Beer

Front 13

Can two atoms be isoelectronic with each other?

Back 13

NO, however an ion of an element can be isoelectronic with another atom or ion.

i.e. Rb(+) is Isoelectronic with Kr.

Front 14

What does Isoelectronic refer to?

Back 14

It refers to two ions or atoms having the same # of electrons.

Front 15

Can an ion have the same electron configuration as an atom of a different element?

Back 15

Yes,

because the electron configuration shows how many electrons are present in an ion or atom. And just as an ion can be isoelectronic with an atom of a different element, so can its electron configuration be the same.

Front 16

What 3 transition elements are exceptions to the Roman numeral Rule?

Back 16

Zinc, Cadmium, Silver

Front 17

What Non-transition metals are an exception to the Roman numeral rule?

Back 17

Tin & Lead

Hint 17

*Remember: these ones have weird prefixes (they use the latin prefix instead of the English ones, they are not hard to miss)

Front 18

What is the difference between Monoatomic and Polyatomic Ions?

Back 18

Monoatomic ions are single atoms with a charge, whereas polyatomic ions are a group of atoms with an overall charge

Front 19

True or False?

When expressing a formula-unit in writing, you should write the metal before the non-metal, followed by the word "ion":

i.e. 'Calcium phosphate ion'

Back 19

False,

it is incorrect to express a formula unit as an ion. Once two ions combine to form a formula-unit, they have full valence shells, and are no longer considered ions.

Front 20

True or False?

All atoms with the suffix '-ide' are monoatomic ions, and should be written with this suffix when expressed in a molecular formula.

Back 20

True with exceptions;

The exceptions are hydroxide and cyanide, which are polyatomic ions.

Front 21

What suffix is used to express polyatomic ions?

Back 21

"-ate" & "-ite"

Front 22

True or False

If asked to write the name of a formula with a charge, you should always write "ion" following the name.

i.e. Cu(2+)

Back 22

True

= Copper (II) ion

Front 23

True or False?

Diatomic molecules always have the suffix "-ide"

Back 23

True

Front 24

What is the charge of a zinc (Zn) ion?

Back 24

2+

Front 25

What is the charge of a Nickel (Ni) ion?

Back 25

It varies

Front 26

What is the charge of an Aluminum (Al) ion?

Back 26

3+

Front 27

What is the charge of a Lead (pb) ion?

Back 27

it varies

Front 28

What is the charge of a silver (Ag) ion?

Back 28

1+

Front 29

What is the charge of a Cadmium (Cd) ion?

Back 29

2+

Front 30

What are the rules of nomenclature for Covalent Bonds?

Back 30

- add suffix "-ide" to ONLY the second element in the equation

- add prefix that correlates with the # of elements in the equation.

- the prefix "-mono" should NOT be used with 2 exceptions (Carbon monoxide, Nitrogen monoxide)

Front 31

What is the name for this compound?

Br3O7

Back 31

tribromine heptaoxide

Front 32

true or false?

In ionic bonds, the charge ratio of ions always has to be 1:1, but the # of ions in the equation does not have to be 1:1

Back 32

True

Front 33

true or false?

In ionic bonds, the number of ions in the equation has to be 1:1, but the charge ratio of the ions does not have to be 1:1

Back 33

False

Front 34

What is the name of the theory that explains the shapes of molecules?

Back 34

Valence Shell Electron Pair Repulsion Theory

(VSEPR)

Front 35

What are the two types of electrons involved in the VSEPR theory?

Back 35

1 - Non bonding electron pairs (Lone pairs)

2 - Bonding electron pairs

Front 36

According to the VSEPR theory, what determines the shape of molecules?

Back 36

The electron pairs will arrange themselves in space the farthest apart from one another because they are negatively charged

Front 37

What is the general idea of the VSEPR theory?

Back 37

That outer energy level electrons determine the shape of a molecule.

Front 38

What is the shape and bond angle of a methane molecule CH(4)?

Back 38

- tetrahedral (109.5 deg)

Front 39

What is the shape and bond angle of an ammonia molecule NH(3)?

Back 39

- trigonal pyramidal (107 deg)

Front 40

What is the shape and bond angle of a water molecule H(2)O?

Back 40

- Bent (104.5 deg)

Front 41

What is a general rule of thumb for determining if the valence electrons will be spaced at equal distances in a covalent bond?

Back 41

- If the atoms involved in the bond are polar, and if there is a lone pair in the bond, there will be an unequal spacing due to the inconsistency in electron strength.

Front 42

What is the molecular shape and bond angle of CO(2)?

Back 42

- linear (180 deg.)

Front 43

Elctronegativity ________________ from left to right within a period and ______________ from top to bottom within a group.

Back 43

> Increases

> Decreases

Front 44

why is it a good idea to double check the numbers on bonds before naming them?

Back 44

1- they could have been reduced

2- it can be easy to confuse # of atoms in bond with charge, leading to naming the wrong transition element (i.e. Iron II instead of Iron III)

3 - it is a method to double check if a bond is covalent...in case you miss it.

Front 45

name this compound:

Si(2)Br(6)

Back 45

disilicon hexabromide

Front 46

name this compound:

Pb(SO4)2

Back 46

Lead (IV) Sulfate

Hint 46

This is an example of why it's important to check the charges on the formula.

- In this example the formula has been reduced. So you wouldn't know that it refers to Lead (IV) unless you check the charge

Front 47

Define Polar Covalent Bond:

Back 47

> A bond between two or more non or semi-metals

> in which the atoms share one or more pairs of electrons.

> The bond is unequal due to difference in electronegativity, which results in various molecular shapes.

Front 48

what is the covalent prefix for 10?

Back 48

deca

Front 49

what is the covalent prefix for 6?

Back 49

hexa

Front 50

what is the covalent prefix for 9?

Back 50

nona