GEN CHEM 1 | SA3 Reviewer

Note: this is just a combination of all my flashcards, cards will be updated when competencies are out

Ionic Bonding

transfer of valence electron from metal donor and nonmetal recipient due to big differences in electronegativity, has electronegativity difference of 2 or higher

Chemical Bonds

lasting force of attraction between atoms, ions, or molecules that enable the formation of chemical compounds; they bond to achieve stability similar to the eight valence electrons of noble gases, following the octet rule

Valence Electrons

electrons on the outermost shell of an atom, can be identified based on the group of the element (except for helium having 2 electrons despite being a noble gas)

Recognizing Ionic Bonding

it is usually with a metal and nonmetal and the electronegativity difference is greater than 1.9; an electrostatic force of attraction between a cation and anion

Ionic Bond Properties

• solid at room temp

• high melting and boiling points

• conduct electricity

• soluble in water

Ion

atom that has gained a net charge

Cation

formed when atom loses electrons (positive charge)

Anion

formed when an atom gains electrons (negative charge)

Lewis Dot Symbol

used to keep track of valence electrons in the formation of chemical bonds, also used to display ionic and covalent bonds

Writing Formulas for Binary Ionic Bonds

1. Write the chemical symbols of both elements.

2. Determine the ionic charge of both elements, basing it on their groups in the periodic table.

3. Crisscross the ionic charges to be the subscripts so that the charge of one element is the subscript of another.

4. If possible, simplify the subscripts to the smallest ratio

Naming Ionic Compounds

1. Name the metal element.

2. Name the nonmetal element and add the suffix -ide to it

Covalent Bonding

sharing of valence electrons between two nonmetals due to close values of electronegativity

Covalent Bond Properties

• exist as solid, liquid, and gas

• low melting and boiling points

• do not conduct electricity and heat

Recognizing Covalent Bonding

usually between two nonmetals and has an electronegativity difference of 0 to 1.9

Writing Formula of Binary Covalent Compounds

1. Write the chemical symbol based the arrangement of their names.

2. Determine the subscripts based on the given prefix

Writing Names of Binary Covalent Compounds

1. Write the name of the two nonmetals.

2. Add a prefix to both based on the subscripts.

3. Add the suffix -ide at the end of the 2nd nonmetal.

Writing Names of Binary Covalent Compounds with Transition Metals (Stock System)

Cation/Metal (Roman Numeral Representing Charge) + Nonmetal Anion

Writing Names of Binary Covalent Compounds with Transition Metals (Classical System)

For the cation with less charges, use “-ous,” for the cation with more charges use “-ic.” Use the latin name/origin name of the cations.

mono-

1 atom

di-

2 atoms

tri-

3 atoms

tetra

4 atoms

penta

5 atoms

hexa-

6 atoms

hepta-

7 atoms

octa-

8 atoms

nona-

9 atoms

deca-

10 atoms

Metallic Bond

attraction between metallic cation and the sea of delocalized electrons, only between metals

Metallic Bond Properties

• malleable and ductile

• conduct electricity

• manifest hardness and strength

s-orbital

spherical shaped orbital, in energy levels 1-7

p-block

dumbell shaped orbital, in energy levels 2-7

d-block

clover leaf shaped, in energy levels 3-6

f-block

orbital with a complicated shape, in energy levels 4-5

The Latin name of Iron (Fe)

Ferrum

The Latin Name of Copper (Cu)

Cuprum

The Latin name of Iron (Fe)

Ferrum

The Latin name of Antimony (Sb)

Stibium

The Latin name of Gold (Au)

Aurum

The Latin name of Lead (Pb)

Plumbum

The Latin name of Mercury (Hg)

Hydragyrum/Mercury

The Latin name of Potassium (K)

Kalium

The Latin name of Silver (Ag)

Argentum

The Latin name of Sodium (Na)

Natrium

The Latin name of Tin (Sn)

Stannum

The Latin name of Tungsten (W)

Wolfram

Ternary Compound

a compound with three or more atoms, usually has a metallic cation and a polytatomic anion

Naming Ternary Compound

For compounds with more than three elements, combine the names of the metallic cation then the polyatomic anion

Valence Shell Electron Pair Repulsion (VSEPR) Theory

electrons surrounding atoms exert repulsive forces against each other, which means a molecule will take a shape where this will be minimized

Central Atom

Represented by A, it is where all the bonds are attached to.

Electron Groups

consists of bonding groups and lone pairs

Bonding Groups

Represented by X, these are the bonds formed between the central atom and the other atoms

Lone Pairs

Represented by E, these are pairs of electrons that did not form a bond

Linear Electron Geometry

2 electron groups; sp hybridization; 180º

Trigonal Planar Electron Geometry

3 electron groups; sp² hybridization; 120º

Tetrahedral Electron Geometry

4 electron groups; sp³ hybridization; 109.5º

Trigonal Bipyramidal Electron Geometry

5 electron groups; sp³d hybridization and 120º (in plane) and 90º (above and below plane) for all VSPER classes except linear which has 180º

Octahedral Electron Geometry

6 electron groups; sp³d² hybridization and 90º

Linear Molecular Geometry

• AX₂ (2 bonds, 0 lone pairs)

• AX₂E₃ (2 bonds, 3 lone pairs)

• AX₂E₄ (2 bonds, 4 lone pairs)

Trigonal Planar Molecular Geometry

AX₃ (3 bonds, 0 lone pairs)

Bent Molecular Geometry

• AX₂E (2 bonds, 1 lone pair)

• AX₂E₂ (2 bonds, 2 lone pairs)

Tetrahedral Molecular Geometry

AX₄ (4 bonds, 0 lone pairs)

Trigonal Pyramidal Molecular Geometry

AX₃E (3 bonds, 1 lone pair)

Trigonal Bipyramidal Molecular Geometry | Composition

AX₅ (5 bonds, 0 lone pair)

Seesaw Molecular Geometry | Composition

AX₄E (4 bonds, 1 lone pair)

T-Shaped Molecular Geometry | Composition

• AX₃E₂ (3 bonds, 2 lone pairs)

• AX₃E₃ (3 bonds, 3 lone pairs)

Octohedral Molecular Geometry | Composition

AX₆ (6 bonds, 0 lone pairs)

Square Pyramidal Molecular Geometry | Composition

AX₅E (5 bonds, 1 lone pair)

Square Planar Molecular Geometry | Composition

AX₄E₂ (4 bonds, 2 lone pairs)

Predicting Molecular Geometry

1. Draw the Lewis Structure of the molecule

2. Count the number of bonds and lone pairs based on the central atom. Write these as the AXE notation.

3. Determine the shape based on the given notation

4. Draw the molecule based on the shape.

What is the line if the bond is on the plane of the paper?

Straight line

What is the line if the bond is coming out of the page towards us?

Triangle

What is the line if the bond is going into the page away from us?

Broken line

What molecular geometry is shown here?

Linear

What molecular geometry is shown here?

Trigonal Planar

What molecular geometry is shown here?

Bent/Angular

What molecular geometry is shown here?

Tetrahedral

What molecular geometry is shown here?

Trigonal Pyramidal

What molecular geometry is shown here?

Trigonal Bipyramidal

What molecular geometry is shown here?

Seesaw

What molecular geometry is shown here?

T-Shape

What molecular geometry is shown here?

Octahedral

What molecular geometry is shown here?

Square Pyramidal

What molecular geometry is shown here?

Square Planar

What molecular geometry is shown here?

Linear (AX2)

What molecular geometry is shown here?

Trigonal Planar

What molecular geometry is shown here?

Bent

What molecular geometry is shown here?

Tetrahedral

What molecular geometry is shown here?

Trigonal Pyramidal

What molecular geometry is shown here?

Trigonal Bipyramidal

What molecular geometry is shown here?

Seesaw

What molecular geometry is shown here?

T-shape (AX3E2)

What molecular geometry is shown here?

Linear (AX2E3 and AX2E4)

What molecular geometry is shown here?

Octahedral

What molecular geometry is shown here?

Square Pyramidal

What molecular geometry is shown here?

Square Planar

What molecular geometry is shown here?

T-shape (AX3E3)

Electronegativity

ability or tendency of an atom to attract electrons and thus form bonds.

Electronegativity Trends

an element’s electronegativity increases from left to right and bottom to top of the periodic table

Nonpolar Covalent Bond

there is equal sharing of electrons between atoms; electronegativity difference is less than 0.5