Chemical Bonding and other stuff for test

Question 1

Octet rule

Answer 1

Atoms form bonds in order to attain stability and the electron configuration of the nearest noble gas

Question 2

Stable octet

Answer 2

All orbitals are completely filled in outermost energy level, noble gases have this, s and p orbitals filled, 8 electrons

Question 3

What are the types of chemical bonds

Answer 3

Ionic, covalent, metallic

Question 4

Ionic bond

Answer 4

Due to transfer of electrons

Question 5

Covalent bond

Answer 5

Due to sharing of electrons

Question 6

Metallic bond

Answer 6

Due to attraction of metallic cations for delocalized electrons

Question 7

What are properties of ionic bond

Answer 7

Result from electrostatic (refers to interaction between charges + and -) interactions among ions
Formed by transfer of electrons between atoms or groups of atoms
Occur between metals and Nonmetals or polyatomic ions (cations smaller than original atom)

Question 8

Properties of covalent bond

Answer 8

(Together, outer electron)
Results from sharing electrons between atoms
Occur between Nonmetals (form molecules ?)

Question 9

Molecules

Answer 9

Neutral groups of atoms held together by covalent bond

Question 10

Ion

Answer 10

Charged particle, while molecule is neutral

Question 11

Neutral

Answer 11

Protons and neutrons cancel each other out / balance each other / equal

Question 12

What are the kinds of covalent bonds

Answer 12

Single covalent bond, double covalent bond, triple covalent bond

Question 13

Single covalent bond

Answer 13

Two atoms share two electrons

Represented: -

Question 14

Double covalent bond

Answer 14

2 atoms share 4 electrons

Rep: =

Question 15

Triple covalent bond

Answer 15

-
- rep

Question 16

What are metallic bond properties

Answer 16

Delocalized electrons in this
Results from the electrical attractions among positively charged metal ions (metal cations) and mobile delocalized electrons

Question 17

Ionic compound properties

Answer 17

High melting point temperatures due to fixed arrangement of ions
Many are soluble (dissolve) in polar solvents (substance that dissolves something else) such as water (which is a polar solvent)
Most are insoluble in no polar solvents such as hexane (nonpolar solvent) (C6H14h
Molten (melting) compounds conduct electricity well
Aqueous (dissolves in water) solutions conduct electricity well

Question 18

Conclusions about ionic compounds based on properties

Answer 18

Have specific crystalline structures (exist as crystalline solids)
Interact with polar substances because of ionic charges
Do not interact with nonpolar substances bc of ionic charges
Conduct electricity when ions are able to move (have to be able to move)

Question 19

Covalent compound properties

Answer 19

Exist as gases, liquids, or low melting solids (powdery, easier to break than ionic compound)
Many are insoluble in polar solvents (opposite ionic)
Most are soluble in nonpolar solvents ( opp ionic)
Molten compounds do not conduct electricity
Aqueous solutions are poor conductors of electricity bc most do not contain charged particles
Covalent=molecule=neutral=can’t conduct electricity

Question 20

Conclusions based on covalent compound properties

Answer 20

Atomic arrangements are not as ordered as ionic compounds
Don’t interact with polar solvents bc they don’t contain charges
Do interact with nonpolar solvents bc they have similar structures
Don’t conduct electricity well because they aren’t composed of charges

Question 21

Metallic properties

Answer 21

Almost all are solids
Have a metallic luster
Are malleable (can be hammered into sheets)
Are ductile (can be drawn into wires, can apply pressure to it and it won’t break)
Have high thermal and electrical conductivity

Question 22

Conclusions based on metallic properties

Answer 22

Exist as solids bc the atoms are in an ordered arrangement
Are malleable and ductile because of the mobility of the electrons
Conduct heat and electricity bc of the mobility of electrons (electrons aren’t attracted to metal but around it, so they are more mobile)

Question 23

Electronegativity

Answer 23

The ability of an atom in a molecule to attract shared electrons to itself

Question 24

Polarity

Answer 24

The unequal distribution of electrons

Question 25

Electronegativity and bond type

Answer 25

The greater the Electronegativity difference in atoms, the more polar the bond

Question 26

Electronegativity difference and bond type chart

Answer 26

2.0= ionic

Question 27

Chemical bond

Answer 27

Attractive force that holds atoms together in compounds

Question 28

Lewis structures

Answer 28

Diagram showing how valence electrons are arranged among the atoms in a molecule

Question 29

Electron dot structure

Answer 29

Represent 1 atom Shows valence electrons Group #= valence electron for groups 1,2, 13, -18

Question 30

Rules for Lewis structure

Answer 30

Hydrogen and halogens share a max of 2 electrons (form only single bonds, never in middle of things) Group 14 elements share max of 8 electrons Group 15 share a max of 6 electrons (tend to form three bonds) Group 16 elements share a max of 4 electrons

Question 31

Dots | Lines

Answer 31

No bonding /unshared electrons | Shared electrons

Question 32

Memorize ...

Answer 32

Lewis structure chart

Question 33

Common bonding configurations

Answer 33

Central atoms are obeying octet rule

Question 34

When drawing Lewis structures

Answer 34

The atoms that form the most bonds goes in the middle of structure

Question 35

Molecular shapes

Answer 35

The three dimensional arrangement of atoms in a molecule

Question 36

What does vsepr stand for

Answer 36

Valence, shell, electron, pair, repulsion

Question 37

What is the vsepr theory?

Answer 37

Shape is determined by presence or absence of unshared electrons in central atom Building toward repulsion Molecules adjust their shapes so that valence electron pairs are as far apart as possible

Question 38

Unshared electrons occupy...

Answer 38

More space than shared electrons | Building toward repulsion

Question 39

Electronic geometry

Answer 39

The arrangement of valence electrons around a central atom

Question 40

Molecular geometry

Answer 40

The arrangement of atoms around a central atom

Question 41

Basic molecular geometries

Answer 41

``` Linear Trigonal planer Bent Pyramidal Trigonal bipyramidal Tetrahedral Octahedral ```

Question 42

Linear

Answer 42

Atoms in a straight line All diatomic molecules are linear Triatomic molecules are linear if the central atom has no unshared electrons Bond angle- 180 Central atom doesn't have unshared electrons Electronic geometry- linear Ex- carbon dioxide (CO2)

Question 43

Trigonometry planer

Answer 43

3 atoms bonded to 1 central atom all in the same plane No unshared e Molecule is flat Exceptions to octet rule (central atom has more or less valence e than 8) Most common central atom for this model is boron Bond angle- 120 Electronic geo- trigonal planer Ex- bf3 BCl3

Question 44

Bent

Answer 44

2 atoms bonded to one central atom all in the same plane There are unshared e on central atom Molecule is flat Bond angle- 104.5 Electronic geo- tetrahedral (4 pairs of electrons around central atoms) # of atoms around central atoms and e aren't the same, so shapes will be different

Question 45

Pyramidal

Answer 45

``` 3 atoms bonded to one central atom There are unshared e on central atom Bond angle- 107 Electronic geo- tetrahedral (4 pairs of e) Ex ammonia (NH3) ```

Question 46

Tetrahedral

Answer 46

``` 4 atoms bonded to 1 central atom No unshared e on central atom Bond angle- 109 Electronic geo- tetrahedral (matches) Ex- methane (CH4) ```

Question 47

Trigonal Bipyramidal

Answer 47

``` 5 atoms bonded to 1 central atom No unshared e on central atom Are exceptions to octet rule Bond angle -90, 120, 180 Electronic geo- trigonal bipyramidal Ex- PF5 ```

Question 48

Octahedral

Answer 48

``` 6 atoms bonded to 1 central atom No unshared e on central atom Are exceptions to octet rule (not rare) Bond angle- 90, 180 Electronic geo- octahedral ```

Question 49

Study picture examples of molecular shapes

Answer 49

Yay!

Question 50

Connect ideas and info!

Answer 50

You got this!