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A Chem 101 2025 & Bond Types > Bond Types > Flashcards

Bond Types Flashcards

1
Q

What type of bond does anything with Hydrogen always form?

A

Polar covalent

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2
Q

What type of bond is created between Carbon and Carbon

A

Pure covalent = same atoms

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3
Q

What the difference between electron affinity and electron negativity

A

Electron Negativity = sharing electrons pulling strongly 1 way or another way.

Electron Affinity = gaining electrons

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4
Q

What forms an ionic bond?

A

A metal and a non-metal

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5
Q

What type of bond is formed between Carbon and Hydrogen

A

Polar Covalent

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6
Q

What is the discrepancy in valence bond theory?

A

O2, - diamagnetic bc all e- are paired which means it repels a magnet a

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7
Q

Describe Hybridization

A
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8
Q

If something attracts a magnet, it is considered

A

Paramagnetic

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9
Q

If something repels a magnet, it is considered

A

Diamagnetic

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10
Q

Assumes electrons occupy atomic orbitals of individual atoms; individual atoms participate in forming bonds

A

Valence Bond Theory (VB)

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11
Q

Atomic orbitals form molecular bonds

A

Molecular Orbital (MO) Theory

  • better describes magnetic & some other properties
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12
Q
A
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13
Q

What elements do we draw Lewis Dot Diagrams for?

A

Everything but:

Transition Metals
& Lanthanides & Actinides - at bottom of Periodic Table

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14
Q

Lewis Dot Symbols for all Elements Groups 1A-8A of the Periodic Table

A
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15
Q

Electrostatic Force that holds ions together in an ionic compound is called

A

Ionic Bonding

Electrostatic Force means positive & negative

We know ions are positive & negative

Li + F —> LiF (Lithium Flouride)

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16
Q

Li + F —> LiF (Lithium Flouride)

Lithium ionizes

A

1st ionization energy of Lithium
Li(0) —> Li+1 (lost electron)
Elemental —> compound

1st Electron Affinity of Flourine (acceptance of electron by Flourine)

F(0)—> F-1 Elemental—> compound

Both full outer shell now, both stable

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17
Q

The energy needed to completely separate, 1 mol of a solid ionic compound into gaseous ions is called?

A

Lattice Energy
- used to measure the stability of ionic solids
- higher lattice energy means it is STABLE & requires more energy to break it apart

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18
Q

Higher LATTICE ENERGY means

A

More STABILITY

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19
Q

What is a bond in which 2 ELECTRONS are SHARED by 2 ATOMS

A

Covalent Bond
(Represented by a dash rather than dots)

The electrons represented by a Covalent Bond are called BONDING ELECTRONS

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20
Q

What do COVALENT BONDS represent?

A

2 BONDING electrons

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21
Q

What elements are involved in COVALENT BONDS? (Shared e- bonds)

A

Non-Metals

(Not the middle transition metals & not the staircase)

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22
Q

What is ionic bonding?

A

Electrostatic force that holds ions together in an ionic compound
(Positive & negative)

Li+ + F- —> LiF (Lithium Fluoride)

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23
Q

In order for lithium and fluorine to bond lithium must? And fluorine must?

A

Lithium must -lose an electron
& go from 0 to +1
(Ionization of Lithium)

Fluorine must- gain an electron
& go from 0 to -1
(Electron Affinity of Fluorine)

(Add these 2 steps to figure out the total energy need for this process)

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24
Q

Lewis Dot Diagrams for Lithium Fluoride

A

Lithium - 1 dot
Fluoride - 7 dots, join to make a full octet

Lithium +1 has no dots (no negatives)
Fluorine gained an electron from Lithium and they achieved a full octet

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25
Energy needed to completely separate, 1 mole of a solid ionic compound into gaseous ion
Lattice Energy - Used to measure the STABILITY of ionic solids - higher lattice energy means more energy to break it apart so if it requires a HIGHER LATTICE ENERGY - it is STABLE and doesn’t want to be broken apart
26
Lattice Energy is
Stability of an ion - the harder they are to break apart, the more stable they are -higher lattice energy = high stability
27
What is COVALENT bonding?
When electrons are shared by 2 atoms Co-valent = shared valence e- Co parenting = shared parenting 1 dash = 2 dots (aka 2 shared electrons) Bonding electrons
28
When 2 F- atoms try to join together
Covalent Bonds are when non-metals try to react with other non-metals If F- join together by sharing 2 electrons Becomes F2- covalent bond- diatomic molecule F—F (2 electrons shared for F2)
29
Electrons around an atom that are not covalently bonded are called
Lone Pairs Or non-bonding electrons —are not involved in covalent bonding
30
When you take 2 Lewis Dot Symbols and put them together with shared electrons, you create ____________?
A Lewis Structure
31
Structure as in Lewis STRUCTURE applies to ________ and __________?
Compounds & molecules
32
What is A representation of covalent bonding in which shared electron pairs are shown as lines or pairs of dots between atoms, lone pairs are shown as pairs of dots on individual atoms, called?
Lewis Structures
33
What are the three forms of covalent bonds?
Single Bonds (1 covalent bond) Double Bonds (2 covalent bonds) Triple Bonds (3 covalent bonds)
34
Bond Length is?
The distance between the nuclei of two covalently bonded atoms Single bond = longest & least stable Triple Bond = shortest & most stable
35
36
Ionic bond is formed by?
A metal and nonmetal Cation & Anion
37
Covalent bonds are formed by?
2 non-metals 2 things on right side of Periodic Table
38
Are ionic compounds considered electrolytes?
Yes, strong electrolytes
39
Ionic Bonds VS. Covalent Bonds
40
The ability of an atom to ATTRACT ELECTRONS (E-) in a CHEMICAL BOND towards ITSELF is called its
ELECTRONEGATIVITY Attract negative electrons to itself
41
42
Covalent bonds made up of 2 of the same atoms like H—H or F—F, how are the electrons shared??
EQUALLY The atoms have equal pull on the electrons and the electrons would be located in the direct center between them
43
If a Covalent Bond is made up of 2 DIFFERENT atoms, how are the electrons shared?
H—F Electrons are not shared equally. 1 of these atoms will have a stronger pull on the electrons Creating a POLAR BOND
44
45
What creates a POLAR BOND?
When Electrons are NOT shared equally, 1 of these atoms will have a stronger pull on the electrons
46
How does electronegativity increase?
Up and to the right Bottom to top Left to right
47
Electronegativity trend stops at ?
Group 7 Halogens b/c Group 8 Noble Gases don’t participate in bonding Element furthers up to right that participates in covalent bonding is Fluorine - highest electronegativity Francium- smallest electronegativity
48
Which element can pull electrons more than any other element?
Fluorine
49
What can electronegativity be used to determine?
The types of bonds between two atoms
50
When bonds are made up of the same element, like : H—H, O—O, F—F they are:
PURE or NonPolar Covalent -Bonds are shared equally between atoms
51
Atoms of elements with similar electronegativities like O-Cl, N-O Create what type of bonds?
Polar Covalent Bonds Covalent- shares electrons Polar- (electrons are shared UNEQUALLY) Polar opposite electron sharing
52
Atoms of elements with widely different electronegativities create what type of bond?
IONIC bond NaCl KBr
53
Similar electonegativities are going to be close to each other on the table like
2 non-metals
54
Different electronegativities would be located where?
Opposite sides of the periodic table IONIC BONDS
55
Elements that are different but next to each other on the periodic table, like groups 6&7, create what type of bond?
Polar Covalent (Different non-metals / share electrons )
56
General rule of thumb for creating an ionic bond is:
Polar Opposites Electronegativity difference is 1.9+ or more Ex. HCl H=2.1 Cl=3.0 Subtract = .9 so it cannot be ionic
57
Bonds between the same element has to be what type of bond?
Pure Or non polar covalent Non-polar= not opposite (the same) Covalent = shared electrons
58
What does non polar mean?
The same or similar
59
What does covalent mean?
Shared valence electrons
60
Ionic bonds create
+1 -1 bonds Conduct electricity in solution & soluble in water, high boiling & melting points
61
Polar covalent bonds
Share e- And have different electronegativities
62
Pure covalent (non-polar)
Bonds that share electrons with atoms of the same molecule or similar
63
What type of bond does Hydrogen create with group 7 Halogens?
NOT IONIC polar covalent bonds from hydrogen
64
What is the difference between electronegativity and electron affinity?
Electron AFFINITY is an isolated atom’s ability to GAIN an electron Electron NEGATIVITY is the ability of an atom within a bond to ATTRACT electrons towards itself
65
Where do Hydrogen and Fluorine go on Lewis Structures?
The ends
66
Which atom goes in the center of a Lewis structure?
67
HYBRIDIZATION is a fundamental concept that helps explain how atoms combine to form molecules with specific shapes and bonding characteristics. DESCRIBE HYBRIDIZATION
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. This process is essential for understanding the bonding and geometry of molecules. Here are the key points about hybridization: 1. **Atomic Orbitals**: Atoms have various atomic orbitals (s, p, d, f) that can hold electrons. In the bonding process, these orbitals can mix or hybridize to create new orbitals. 2. **Hybrid Orbitals**: The new orbitals formed through hybridization are called hybrid orbitals. They have different shapes and energies compared to the original atomic orbitals. The most common types of hybridization are: - **sp Hybridization**: Involves one s orbital and one p orbital, resulting in two equivalent sp hybrid orbitals. This type of hybridization typically leads to linear geometry (180° bond angles). - **sp² Hybridization**: Involves one s orbital and two p orbitals, resulting in three equivalent sp² hybrid orbitals. This leads to trigonal planar geometry (120° bond angles). - **sp³ Hybridization**: Involves one s orbital and three p orbitals, resulting in four equivalent sp³ hybrid orbitals. This leads to tetrahedral geometry (109.5° bond angles). - **sp³d Hybridization**: Involves one s orbital, three p orbitals, and one d orbital, resulting in five equivalent sp³d hybrid orbitals. This is typical for trigonal bipyramidal geometry. - **sp³d² Hybridization**: Involves one s orbital, three p orbitals, and two d orbitals, resulting in six equivalent sp³d² hybrid orbitals, leading to octahedral geometry. 3. **Bonding and Geometry**: Hybridization helps explain the observed shapes of molecules based on the arrangement of the hybrid orbitals around the central atom. For example, methane (CH₄) has a tetrahedral shape due to sp³ hybridization. 4. **Sigma and Pi Bonds**: Hybrid orbitals typically form sigma (σ) bonds through head-on overlap with other orbitals. Pi (π) bonds, on the other hand, are formed from the side-to-side overlap of unhybridized p orbitals. 5. **Applications**: Understanding hybridization is crucial in predicting molecular geometry, reactivity, and the properties of compounds in organic and inorganic chemistry.
68
The formal charge helps to determine the most stable Lewis structure for a molecule, as the best structure typically has the smallest formal charges on the atoms. How do you calculate the formal charge?
The formal charge of an atom in a molecule can be calculated using the following formula: [ \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons} ] Here’s how to apply the formula: 1. Valence Electrons: Determine the number of valence electrons for the atom in its neutral state (based on its group number in the periodic table). 2. Non-bonding Electrons: Count the number of non-bonding (lone pair) electrons that are associated with the atom. 3. Bonding Electrons: Count the total number of electrons that are shared in bonds with other atoms. Since each bond involves two electrons, you will take half of this number. 4. Plug Values into the Formula: Substitute the values into the formula to find the formal charge.
69
What geometry name, AB designation, and bond angles are involved in B—A—B ?
Linear AB2 180degrees
70
What geometry name, AB designation, and bond angles are involved in B A B B B
Tetrahedral AB4 109.5 degrees
71
What geometry name, AB designation, and bond angles are involved in
Distorted Tetrahedron (Seesaw) AB4E1 Less than 120 degrees
72
What geometry name, AB designation, and bond angles are involved in B A B B
Trigonal Planar AB3 120 degrees
73
What geometry name, AB designation, and bond angles are involved in LP A B B
Bent AB2E1 Less than 120degrees LP= lone pair
74
What geometry name, AB designation, and bond angles are involved in LP A B B B
Trigonal Pyramidal AB3E1 Less than 109.5degrees
75
What geometry name, AB designation, and bond angles are involved in LP A LP B B
Bent AB2E2 Less than 90degrees
76
77
What geometry name, AB designation, and bond angles are involved in
Trigonal Bipyramidal AB5 90 degrees & 120 degrees
78
What geometry name, AB designation, and bond angles are involved in
T-shaped AB3E2 Less than 90 degrees
79
What geometry name, AB designation, and bond angles are involved in
Linear AB2E3 180 degrees
80
What geometry name, AB designation, and bond angles are involved in
Square Pyramidal AB5E1 Less than 90 degrees
81

A Chem 101 2025 & Bond Types (6 decks)

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