Chemistry-Test 2 Chapter 4

Front 1

Most compounds that we come in contact with in our daily lives are ___________________.

Back 1

Covalent Compounds

Front 2

Formed by sharing electrons between atoms?

Back 2

Covalent Compounds

Front 3

-Air we breathe

-Body is mostly water

-Drugs (asprin acetaminophen, ibuprofen, all antibiotics)

-Products of chemical industry (polyethylene, nylon, synthetic dyes, gasoline, and pesticides)

THESE ARE ALL EXAMPLES OF?

Back 3

Covalent Compounds

Front 4

A two electron bond in which the bonding atoms share valence electrons?

Back 4

Covalent Bond

Front 5

A discrete group of atoms held together by covalent bonds?

Back 5

Molecule

Front 6

Solid line between two element symbols to represent a _______-electron bond.

Back 6

Two

Front 7

Only contain two atoms? and Which element is this?

Back 7

-Diatomic Molecules

-Hydrogen

Front 8

Unshared electron pairs are called?

Back 8

Lone Pairs (nonbonded electron pairs)

Front 9

Covalent bonds are formed when two ____________ combine. Also formed when a ______________ bonds to a ____________.

Back 9

-Nonmetals

-Metalloid

-Nonmetal

Front 10

___________ is a main component of natural gas. __________ is in agricultural fertilizer. ___________ is also another example of covalent molecules in which each main group element is surrounded by 8 electrons.

Back 10

-Methane

-Nitrogen

-Oxygen

Front 11

Electron-dot structure for molecules are called?

Back 11

Lewis Structures

Front 12

Show the location of all valence electrons in a molecule, both the shared electrons in the bonds, and the non-bonded electron pairs?

Back 12

Lewis Structures

Front 13

Atoms with one, two, or three valence electrons generally form one, two, or three bonds respectively. Atoms with four or more valence electrons form enough bonds to give an ___________.

Back 13

Octet

Front 14

________ is the most prevalent covalent compound in the body; Oxygen is carried by the protein ______________ to the tissues; Glycine is a building block of the proteins that compose heart muscle; Nitroglycerin is a drug used to treat some forms of ______________.

Back 14

-Water

-Hemoglobin

-Heart disease

Front 15

A ______________ formula ONLY shows the number and identity of all of the atoms in a covalent compound.

Back 15

Molecular

Front 16

A _____________, shows the connectivity between the atoms, as well as where all the bonding and nonbonding valence electrons reside.

Back 16

Lewis Structure

Front 17

Rules for drawing Lewis Structures: draw only the ____________ electrons. Give every main group element an ___________ (except hydrogen). Give each hydrogen _______ electrons.

Back 17

-Valence

-Octet

-2

Front 18

Contain 6 electrons in three two-electron bonds?

Back 18

Triple Bond

Front 19

Contain 4 electrons in two two-electron bonds?

Back 19

Double Bond

Front 20

Carbon, Nitrogen, Oxygen, and Halogens are the most common elements of?

Back 20

Covalent Compounds

Front 21

4 elements that do not follow the octet rule?

Back 21

-Hydrogen (not enough)

-Boron (not enough)

-Phosphorus (more than 8)

-Sulfur (more than 8)

(do not have enough valence electrons to form an octet in a neutral molecule)

Front 22

In counting valence electrons, _______ one electron for each negative charge. _________ one electron for each positive charge.

Back 22

-Add (for neg)

-Subtract (for pos)

Front 23

Two Lewis structures having the same arrangement of atoms but a different arrangement of electrons?

Back 23

Resonance Structures

Front 24

Two resonance structures differ in the ______________ of multiple bonds and the position of the ______________.

Back 24

-Location

-Lone pairs

Front 25

Composite of both resonance forms?

Back 25

Hybrid

Front 26

_____________ stabilizes a molecule by spreading out lone pairs and electron pairs in multiple bonds over a larger region of space.

Back 26

Resonance

Front 27

Molecule or ion that has two or more resonance structures?

Back 27

Resonance-stabilized

Front 28

Resonance structures can be drawn for neutral molecules as well. For example?

Back 28

Ozone (O3)

Front 29

We can use a Lewis structure to determine the ________ around a particular atom in a molecule. To determine this, we must first determine how many ________ surround the atom.

Back 29

-Shape

-Groups

Front 30

Either an atom or a lone pair of electrons?

Back 30

Group

Front 31

Used to determine the shape around a given atom. Based on the fact that electron pairs repel each other?

Back 31

VSEPR

Front 32

The most __________ arrangements keep groups as far away from each other as possible.

Back 32

Stable

Front 33

An atom surrounded by two groups is _______ and has a bond angle of _______ degrees. An atom surrounded by three groups is a _________________ and has bond angles of ________ degrees. An atom surrounded by four groups is _______________ and has bond angles of _________ degrees.

Back 33

-2= linear, 180

-3= trigonal planar, 120

-4= tetrahedral, 109.5

Front 34

VSEPR theory: ignore __________ bonds in predicting geometry. Count only atoms and _______________.

Back 34

-Multiple

-Lone pairs

Front 35

_________ line for bonds in plane. _________ for bond in front of plane. _________ for behind the plane.

Back 35

-Solid line

-Wedge

-Dashed line

Front 36

Geometric shape when one of the groups around the center element is a non bonded electron pair, not another atom?

Back 36

Trigonal Pyramid

Front 37

Measure of an atom's attraction for electrons in a bond. Tells us how much a particular atom "wants" electrons?

Back 37

Electronegativity

Front 38

The higher the value, the _________ electronegative an atom is and the more it is ____________ to the electrons in a bond. Electronegativity values exhibit __________ trends. Electronegativity INCREASES across a _______ of the periodic table as nuclear charges increase (excludes _______________). Electronegativity DECREASES down a __________ of the periodic table as the atomic radius increases, pushing the valence electrons farther from the nucleus.

Back 38

-More

-Attracted

-Periodic

-Row

-Noble Gases

-Column

Front 39

_________ have high electronegativity values because they have a strong tendency to hold on to and attract electrons. _______ have low electronegativity values. Most electronegative elements are ___________ and __________ located in the upper-right corner.

Back 39

-Nonmetal=high

-Metal=low

-Fluorine

-Oxygen

Front 40

Electronegativity values are used as a guideline to indicate whether the electrons in a bond are equally or unequally shared between two atoms. Equally shared means they are ___________. Not equally shared means they are ____________.

Back 40

-Nonpolar

-Polar

Front 41

Partial separation of a charge?

Back 41

Dipole

Front 42

The direction of polarity in a bond is often indicated by a ________, with the head of it poiting toward the _________ electronegative element. The _______ of the arrow, with a perpendicular line drawn through it, is drawn at the _______ electronegative element. Symbol _______ is given to the less electronegative element. Symbol _______ is given to the more electronegative element.

Back 42

-Arrow

-More

-Tail

-Less

-Delta +

-Delta -

Front 43

ELECTRONEGATIVITY DIFF:

Less than 0.5 units is _____________. 0.5-0.9 units is _______________. Greater than 1.9 units is ______________.

Back 43

-Nonpolar

-Polar Covalent

-Ionic

Front 44

Electrons are equally shared in ___________ bond.

Back 44

Nonpolar

Front 45

Electrons are unequally shared in this bond. They are pulled towards the more electronegative element?

Back 45

Polar Covalent

Front 46

Electrons are transferred from the less electronegative element to the more electronegative element in this bond?

Back 46

Ionic

Front 47

Whether an entire covalent molecule is polar or nonpolar depends on _____________ and _____________.

Back 47

-Polarity

-Overall shape

Front 48

Covalent compounds with more than one polar bond, the ________ of the molecule determines the overall polarity. If the individual bond dipoles do not cancel, the molecule is ____________. If they do cancel, the molecule is ___________.

Back 48

-Polar

-Non polar

Front 49

To determine the polarity of a molecule that has two or more polar bonds: Identify all polar bonds based on electronegativity differences. Determine the shape around individual atoms by counting groups. Decide if individual dipoles can cancel or reinforce ***

Back 49

***

Front 50

Covalent molecule used to disinfect wounds? Covalent molecule used as a pain reliever and antipyretic (an agent that reduces fever)?

Back 50

-Hydrogen Peroxide (H2O2)

-Acetaminophen