Chem Test 2

Front 1

What is a chemical bond?

Back 1

A strong attractive force between atoms or ions in a chemical compound

Front 2

__________ elements have relatively high potential energy?

Back 2

Uncombined

Front 3

In order to chemically combine with other atoms, what will atoms do?

Back 3

Gain, lose or share valence electrons

Front 4

What happens to the potential energy of atoms when they combine with other atoms?

Back 4

The PE decreases

Front 5

What two factors determine whether or not a chemical bond will form?

Back 5

Electron configuration and the attraction the atoms have for electrons.

Front 6

What are the types of chemical bonds?

Back 6

Polar and non-polar covalent and ionic.

Front 7

How are electrons shared in a non-polar covalent bond?

Back 7

Equally.

Front 8

In a ____________ bond, electrons are shared unequally

Back 8

Polar covalent

Front 9

Name the diatomic atoms

Back 9

Hydrogen, bromine, oxygen, nitrogen, chlorine, iodine and fluorine.

Front 10

In what type of bond are electrons transferred between atoms?

Back 10

Ionic

Front 11

What do we call a negative ion?

Back 11

Anion

Front 12

What is a cation (cat-ion)?

Back 12

A positively charged ion

Front 13

Anions are typically _________ while cations are typically __________.

Back 13

Anions are non metals, cations are metals

Hint 13

Metallic character

Front 14

What is electronegativity?

Back 14

A measure of an atom or fuctional groups ability to attract electrons when chemically combining with another element.

Front 15

The ________ the electronegativity, the stronger the attraction the atom has for another atoms electrons.

Back 15

Higher

Front 16

How do we determine the degree to which bonding between atoms is ionic or covalent?

Back 16

By calculating the difference in the elements electronegativities (🔺️EN)

Front 17

If the difference in electronegativity is less than 0.2, what type of bond do we have?

Back 17

Nonpolar covalent

Front 18

What is the range for difference in electronegativity for a polar covalent bond?

Back 18

0.2 to 1.7

Front 19

A(n) _______ bond has an electronegativity difference of greater than 1.7.

Back 19

Ionic

Front 20

An atoms electronegativity is affected by both its __________ and the distance at which its ___________ reside from the nucleus.

Back 20

Atomic number and valence electrons.

Front 21

When did Linus Pauling propose his electronegativity scale?

Back 21

1932

Front 22

The periodic table of electronegativity is also called what?

Back 22

The Linus Pauling scale.

Front 23

What is a dipole?

Back 23

A covalent bond between atoms which are not shared equally.

Front 24

The positive dipole in a polar covalent bond would have a ________ electronegativity value.

Back 24

Lower

Front 25

Elements that exist as two atoms chemically bonded are called?

Back 25

Diatomic elements.

Front 26

The bond between diatomic elements is always?

Back 26

Nonpolar covalent.

Front 27

What is VSEPR theory?

Back 27

Valence Shell Electron Pair Repulsion theory.

Front 28

What do we use to predict the 3D shapes of a molecule?

Back 28

VSEPR theory

Front 29

What two tools do we use to determine final molecular shape?

Back 29

VSEPR and Lewis Dot Formula

Front 30

What is the main concept of VSEPR?

Back 30

That election pairs will orient themselves so that repulsion between electron pairs are minimized.

Front 31

What are the molecular shapes? (There are 8)

Back 31

2-atom linear, 3-atom linear, bent, trigonal planar, trigonal pyramidal, tetrahedral, trigonal bipyrimidal, and octahedral.

Front 32

What causes a bent molecular shape?

Back 32

The presence of non bonding electrons in the central atom.

Front 33

How do you differentiate between linear and bent molecules?

Back 33

Linear do not have nonbonding electrons on the central atom, bent molecules do.

Front 34

How do you differentiate between trigonal planar and trigonal pyramidal molecules?

Back 34

Planar molecules do not have non bonding electrons on the central atom, pyramidal do.

Front 35

What two things determine the polarity of a molecule?

Back 35

The polarity of the bond along with the geometry of the molecule.

Front 36

A nonpolar molecule has ________ distribution of molecular charge.

Back 36

Even

Front 37

What type of molecule has an uneven distribution of molecular charge?

Back 37

Polar

Front 38

Which two molecular shapes are always polar?

Back 38

Bent and trigonal pyramidal.