Unit A: Bonding

Question 1

What is the primary type of bond formed between metals and nonmetals?

Answer 1

Ionic bond

Question 2

True or False: Covalent bonds involve the transfer of electrons.

Answer 2

False

Question 3

Fill in the blank: A bond formed by the sharing of electrons is called a __________ bond.

Answer 3

Covalent

Question 4

What type of bond is characterized by a sea of delocalized electrons?

Answer 4

Metallic bond

Question 5

Which type of bonding is typically stronger: ionic or covalent?

Answer 5

Covalent

Question 6

What is a molecule?

Answer 6

A group of atoms bonded together.

Question 7

What do you call the energy required to break a bond?

Answer 7

Bond dissociation energy

Question 8

True or False: Ionic compounds usually have high melting and boiling points.

Answer 8

True

Question 9

What is the octet rule?

Answer 9

Atoms tend to form bonds until they are surrounded by eight valence electrons.

Question 10

Identify the bond type: NaCl.

Answer 10

Ionic bond

Question 11

What type of bond is formed between two nonmetals?

Answer 11

Covalent bond

Question 12

Which bond type usually occurs between metals?

Answer 12

Metallic bond

Question 13

Fill in the blank: The __________ model explains how metallic bonds work.

Answer 13

Sea of electrons

Question 14

True or False: A polar covalent bond occurs when electrons are shared equally.

Answer 14

False

Question 15

What is a polar molecule?

Answer 15

A molecule with a partial positive charge on one end and a partial negative charge on the other.

Question 16

What is the difference between a single bond and a double bond?

Answer 16

A single bond shares one pair of electrons, while a double bond shares two pairs.

Question 17

List one property of ionic compounds.

Answer 17

They conduct electricity when dissolved in water.

Question 18

What is the significance of electronegativity in bonding?

Answer 18

It determines how strongly an atom attracts electrons in a bond.

Question 19

What is a Lewis dot structure?

Answer 19

A diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons.

Question 20

Fill in the blank: The type of bond formed when there is a large difference in electronegativity is called a __________ bond.

Answer 20

Ionic

Question 21

What type of bond occurs in H2O?

Answer 21

Polar covalent bond

Question 22

True or False: Metallic bonds allow metals to be malleable.

Answer 22

True

Question 23

What is the VSEPR theory used for?

Answer 23

To predict the geometry of molecular structures.

Question 24

What is an example of a nonpolar covalent bond?

Answer 24

The bond between two identical nonmetals, like Cl2.

Question 25

What does it mean if a compound is soluble in water?

Answer 25

It can dissolve in water to form a solution.

Question 26

What is an ionic lattice?

Answer 26

A three-dimensional structure of ions held together by electrostatic forces.

Question 27

What is an observation vs an inference?

Answer 27

Observation – knowledge obtained from using the five senses Inference – knowledge that is not directly known; explains an observation

Question 28

What is qualitative vs quantitative?

Answer 28

Qualitative – describes matter Ex. color, odor, state Quantitative – is a quantity of matter; is a number Ex. Measurement of temperature

Question 29

What is the purpose of the atomic diagram: Bhor model and Lewis Model?

Answer 29

Atomic models are used to predict why atoms combine and explain the ratios in which they combine. Lewis: used to explain BONDING Bhor: used to discuss electronegativity and relates to periodic table information

Question 30

What is an orbital?

Answer 30

Orbitals – 3-D space in which an electron of a certain energy should be found Only 0, 1, or 2 electrons can occupy a single orbital (Pauli exclusion principle) 1st energy level = 1 orbital 2nd energy level= 4 orbitals 3rd energy level= 4 orbitals

Question 31

What makes an ion?

Answer 31

When an atom loses (becomes positive) or gains (becomes negative) electrons in order to become stable and like its nearest noble gas. An atom will only ever lose its outermost electrons.

Question 32

What is electronegativity?

Answer 32

Electronegativity - Is the ability of an atom to attract electrons to its valence energy level Higher electronegativity = stronger attraction of electrons

Question 33

What are the three factors that effect electronegativity?

Answer 33

3 Factors That Affect Electronegativity 1. The farther electrons are from the nucleus, the weaker their attraction to their own nucleus IMPLICATION: Going down a family, the electronegativity decreases due to larger # of electrons 2. Electrons close to the nucleus shield (block) attraction of outer electrons - see point #1 IMPLICATION: Down groups, electronegativity decreases (more shielding) 3. The greater # of protons in a nucleus, the stronger the attraction electrons have for their own nucleus IMPLICATION: Across rows, electronegativity increases, because there are more positive protons

Question 34

What is INTRAmolecular bond vs INTERmolecular bonds?

Answer 34

INTRAmolecular bond: Bonding WITHIN molecules (chemical changes) ex. ionic (transfer of electrons) and covalent (sharing of electrons) bonds INTERmolecular bond: Bonding (attraction) BETWEEN molecules (covalent) (physical changes) ex. London dispersion, dipole-dipole, and hydrogen bonds