Bonding

Question 1

When an atom gains or loses an electron they are called…

Answer 1

ions.

Question 2

Metals form what type of ion?

Answer 2

Positive (cation)

Question 3

Non metals form what type of ion?

Answer 3

Negative (anion)

Question 4

What group or groups do not form ions?

Answer 4

4 n 8

Question 5

Transition metals can form many different ions and are usually distinguishable by….

Answer 5

COLOR

Question 6

What is a lattice structure???

Answer 6

They are the 3D shape that ionic compounds take one. When talking about ionic compounds try to avoid the word “molecule” because they don’t form molecules they form a lattice. LATTICE. say it. three times. sounds like lettuce

Question 7

Describe a covalent bond

Answer 7

• between two nonmetals.
• two atoms share electrons. how sweet
• a group of covalent bonds forms a MOLECULE. this is a molecule. covalent bond means molecule. yay

Question 8

Compare and contrast double and triple bonds.

Answer 8

Double bonds have one sigma and one pi bond. Triple have one sigma and two pi bonds. Triple bonds are also stronger and shorter than double bonds.

Question 9

What are dative compounds?

Answer 9

Covalently bonded molecules that are stable but do not follow the octet rule. They react with compounds that have a lone pair (such as H20 or NH3). Examples of dative compounds are BeCl2 and BF3.

Question 10

Describe a polar bond.

Answer 10

This occurs when there is a difference in the electronegativities of bonded atoms. The more electronegative atom pulls the electrons closer to itself creating a polarity.

Question 11

What is the VSEPR theory?

Answer 11

Valence Shell Electron Pair Repulsion. That the shape of a molecule is determined by the repulsion between electron pairs in the outer orbital.

Question 12

Significance of lone pairs (non-bonding pairs of electrons) with regards to the VSEPR theory.

Answer 12

Lone pairs have a higher concentration of charge than a bonding pair and cause more repulsion. Molecules with lone pairs on the central atom have some distortions in their structure which reduce the angle between the bonded angles.

Question 13

Shape and bond angle of molecules with two negative charge centers.

Answer 13

Linear. Bond angle is 180.

Question 14

Shape and bond angle of molecules with three negative charge centers.

Answer 14

Triangular planar, 120

Question 15

Shape and bond angle of molecules with three negative charge centers, but one of the charge centers is a lone pair.

Answer 15

Bent, 117

Question 16

Shape and bond angle of molecules with four negative charge centers.

Answer 16

Tetrahedral, 109.5

Question 17

Shape and bond angle of molecules with four negative charge centers, but one of the charge centers is a lone pair.

Answer 17

Trigonal Pyramidal, 107

Question 18

Shape and bond angle of molecules with four negative charge centers, but two of the charge centers is a lone pair.

Answer 18

Bent, 105

Question 19

Is it possible to have polar bonds within a non-polar molecule.

Answer 19

Yes. Just yes.

Question 20

True or false: some covalent substances form crystalline solids.

Answer 20

True.

Question 21

Describe the crystalline substance.

Answer 21

A single molecule that ha a regular repeating pattern of covalent bonds. Referred to as a giant molecular or MACROMOLECULE.

Question 22

What is an allotrope?

Answer 22

A different for or forms of an element in the same physical state. The different forms are due to different bondings within the structures that result in different shapes and properties.

Question 23

What are the three carbon allotropes.

Answer 23

Graphite
Diamond
Fullerene

Question 24

Describe graphite as an allotrope of carbon.

Answer 24

Each C atom is linked to three more. Forms a hexagons with 120 bond angles. Parallel layers are held by van der waals forces.

Has one delocalized, non bonded electron. Because of that electron it can conduct electricity.

Looks: Dull, gray and solid.

Uses: Found in pencils. Yeeeh

Question 25

Describe diamond as an allotrope of carbon.

Answer 25

Each C atom is covalently bonded to 4 others. They are tetrahedrally arranged in a regularly repetitive pattern of 109.5 bond angles. Hardest known material in existence. All the electrons are bonded. Since there are no floating electrons it cannot conduct electricity. Looks: It is shiny. But seriously. You know what a diamond looks like. Don't be dumb. Uses: jewelry, glass cutter.

Question 26

Describe Fullerene as an allotrope of carbon.

Answer 26

Sphere of 60 carbon atoms. Consists of 12 pentagons and 20 hexagons. Each carbon is bonded to three others. Easily accepts electrons to form negative ions. It is a semiconductor at normal temperature and pressure. Looks: YELLOW crystalline solidl soluble in benzene. Uses: reacts with K to make a super conductor; nanotubes can be made for electronics; catalysts

Question 27

Compare Silicon and silicon dioxide.

Answer 27

Silicon: each silicon atom is covalently bonded to four more. tetrahedral arrangement. Giant lattice structure similar to a diamond. Silicon dioxide: known as silicia or quartz. Forms a giant covalent structure. Si and O are bonded in a tetrahedral shape. Each Si is bonded to 4 O atoms. Each O atom is bonded to 2 Si. It is insoluble in water, does not conduct anything. Different forms are sand and glass.

Question 28

What is an INTERmolecular force? Give three examples.

Answer 28

Forces that exist BETWEEN molecules. Van der Waals' forces Dipole-Dipole attraction Hydrogen Bonding

Question 29

Describe Van der Waals forces

Answer 29

Temporary dipoles form in molecules due to the ever changing electron density. Van der Waals is the attraction between opposite ends of two temporary dipole molecules. Generally, they are weak and easily broken thus molecules with VWF have Low melting points and boiling points. Increasing number of electrons and molecular size will increase the chance of a temporary dipole and the VWF. (larger mass = stronger VFW = higher boiling point)

Question 30

Describe a dipole-dipole attraction.

Answer 30

Typically occurs between molecules that have polar bonds. The delta negative end of one molecule is attracted to the delta positive end of another molecule. Strength varies depending on the degree of polarity

Question 31

Describe hydrogen bonding.

Answer 31

When a molecule containing hydrogen is covalently bonded to FON of another molecules. This bond is a SUPER STRONG dipole dipole attraction. It's so strong it gets its own mf name. Though strong, they are weaker than intramolecular forces such as covalent and ionic bonds. Need a super high boiling point to break. Water is a perf example.

Question 32

What are delocalized electrons? When are they present?

Answer 32

Delocalized electrons are present in the elemental state of a metal. The outer electrons are "loose" and begin to wander through the metal structure. After losing the electron the atom becomes a positive ion and connect with the neighboring positive ions to form a lattice structure. The electrons then move freely through this structure and are able to conduct electricity. The delocalized electrons are able to move any which way. This allows the metal to be malleable (able to be shaped) and ductile (can be drawn into threads).

Question 33

Compare and contrast the boiling and melting points of ionic compounds and covalent compounds.

Answer 33

Ionic compounds = high Giant covalent structures = high Covalent = low

Question 34

Compare and contrast ionic compounds, polar covalent compounds, and non-polar covalent compounds with regard to their solubility in polar solvents and non polar solvents.

Answer 34

Ionic compounds = Soluble in polar, not soluble in non polar. Polar Covalent = solubility increases as polarity increases; solubility increases as polarity decreases. Non-polar covalent - not soluble in polar solvent; soluble in non polar.

Question 35

Compare and contrast ionic compounds, polar covalent compounds, and non-polar covalent compounds with regard to conductivity.

Answer 35

Ionic= As a solid they cannot; in the liquid and molten states they are able Polar = some of them can give n right circumstances (ie HCL in water) NPC = cannot conduct