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Science > Chemical Bonding and other stuff for test > Flashcards

Chemical Bonding and other stuff for test Flashcards

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1
Q

Octet rule

A

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

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2
Q

Stable octet

A

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

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3
Q

What are the types of chemical bonds

A

Ionic, covalent, metallic

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4
Q

Ionic bond

A

Due to transfer of electrons

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5
Q

Covalent bond

A

Due to sharing of electrons

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6
Q

Metallic bond

A

Due to attraction of metallic cations for delocalized electrons

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7
Q

What are properties of ionic bond

A

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)

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8
Q

Properties of covalent bond

A

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

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9
Q

Molecules

A

Neutral groups of atoms held together by covalent bond

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10
Q

Ion

A

Charged particle, while molecule is neutral

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11
Q

Neutral

A

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

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12
Q

What are the kinds of covalent bonds

A

Single covalent bond, double covalent bond, triple covalent bond

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13
Q

Single covalent bond

A

Two atoms share two electrons

Represented: -

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14
Q

Double covalent bond

A

2 atoms share 4 electrons

Rep: =

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15
Q

Triple covalent bond

A

-
- rep

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16
Q

What are metallic bond properties

A

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

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17
Q

Ionic compound properties

A

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

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18
Q

Conclusions about ionic compounds based on properties

A

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)

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19
Q

Covalent compound properties

A

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

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20
Q

Conclusions based on covalent compound properties

A

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

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21
Q

Metallic properties

A

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

22
Q

Conclusions based on metallic properties

A

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)

23
Q

Electronegativity

A

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

24
Q

Polarity

A

The unequal distribution of electrons

25
Q

Electronegativity and bond type

A

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

26
Q

Electronegativity difference and bond type chart

A

2.0= ionic

27
Q

Chemical bond

A

Attractive force that holds atoms together in compounds

28
Q

Lewis structures

A

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

29
Q

Electron dot structure

A

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

30
Q

Rules for Lewis structure

A

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

31
Q

Dots

Lines

A

No bonding /unshared electrons

Shared electrons

32
Q

Memorize …

A

Lewis structure chart

33
Q

Common bonding configurations

A

Central atoms are obeying octet rule

34
Q

When drawing Lewis structures

A

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

35
Q

Molecular shapes

A

The three dimensional arrangement of atoms in a molecule

36
Q

What does vsepr stand for

A

Valence, shell, electron, pair, repulsion

37
Q

What is the vsepr theory?

A

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

38
Q

Unshared electrons occupy…

A

More space than shared electrons

Building toward repulsion

39
Q

Electronic geometry

A

The arrangement of valence electrons around a central atom

40
Q

Molecular geometry

A

The arrangement of atoms around a central atom

41
Q

Basic molecular geometries

A 
Linear
Trigonal planer
Bent
Pyramidal
Trigonal bipyramidal
Tetrahedral
Octahedral
42
Q

Linear

A

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)

43
Q

Trigonometry planer

A

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

44
Q

Bent

A

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

45
Q

Pyramidal

A 
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)
46
Q

Tetrahedral

A 
4 atoms bonded to 1 central atom
No unshared e on central atom
Bond angle- 109
Electronic geo- tetrahedral (matches) 
Ex- methane (CH4)
47
Q

Trigonal Bipyramidal

A 
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
48
Q

Octahedral

A 
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
49
Q

Study picture examples of molecular shapes

A

Yay!

50
Q

Connect ideas and info!

A

You got this!

Science (18 decks)

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