Chapter 3: Molecules, Compounds, and Chemical Equations

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HCO3(-)

Hydrogen Carbonate (bicarbonate)

HSO3 (-)

Hydrogen Sulfate (or bisulfate)

OH(-)

Hydroxide

ClO (-)

Hypochlorite

Iodine

I-

Which of the following is an ionic compound? A. LiCl B. NO2 C. PCl3 D. CF4 E. SeBr2

A

SO3 (-)

Sulfite

Formula mass

Sum of atomic masses o reach element in chemical formula

Molecular

The actual number and types of atoms in a molecule

Anions

Non-metals or polyatomic ions

Cl(O1-)

(Hypo)chlor(ite)

Cl(O4-)

(Per)chlor(ate)

Polyatomic

(many atoms) P4, S8, Se8

Diatomic

(to atoms) N2, O2, F2, Cl2, Br2, I2, H2 (Start at 7 make a 7)

How to name a formula that starts with hydrogen?

1. Add hydro in front the base name of nonmetal 2. Add -ic to -ate; add -ite to -ous (no -hydro if -ite) 3. Add "acid" at the end of the name

Writing Formulas

1. Write symbols and ion charges (periodic table) 2. Charge becomes subscript for the other ion. 3. Reduce subscripts to smallest whole number ratios 4. Check charge neutrality

Molecules

2 or more atoms tightly bonded together When more than one type of atom combines to form a molecule in fixed definite proportions Molecule has different properties than individual elements many elements are found in molecular form

Molecular models

3D representations Ball and stick (modeling kit) Space filling (shows how much space electrons take up)

C2H3O2 (-)

Acetate

NH4 (+)

Ammonium

Covalent

Atoms share electrons and between non-metals

Ionic

Atoms transfer electrons between nonmetals and metal, oppositely charged ions (cation and anions)

Which of the following is an ionic compound? A. SCl2 B. Mg3(PO4)2 C. Cl2O D. CH2O E. PF5

B

Molecular compound is what type of bond?

Covalent

Bromine

Br-

Which of the following contains BOTH ionic and covalent bonds? A. CaI2 B. COS C. CaSO4 D. SF6 E. None of these contain both

C. Calcium is a metal SO4 is a covalent bond

Transition Metals

Can have different charges Use parentheses and numeral to indicate change Ex: CrBr3 Chromium (111) Bromide

CO3(2-)

Carbonate

Cl(O3-)

Chlor(ate)

Cl(O2-)

Chlor(ite)

ClO3 (-)

Chlorate

ClO2 (-)

Chlorite

CrO4(2-)

Chromate

Chlorine

Cl-

Ionic Compounds

Contain both (+) cations and (-) anions charged ions. Formed when 1 or more electrons transfer from one neutral atom to another

CN (-)

Cyanide

Cr2O7(2-)

Dichromate

H2PO4 (-)

Dihydrogen phoshate

CH2O

Empirical formula

Fluorine

F-

Empirical

Gives only the relative number of atom Superscripts with smallest whole number ratios

Chemical Formula

Indicates which atoms are found in the molecule In what proportions they are found (ratio)

Salts (NaCl, Mg3N2)

Ionic Compounds

Structural formula

Lines to represent covalent bonds and shows how atoms are connected Does not describe the arrangement in space (not 3D)

Oxygen

O2-

Cations

Metals or polyatomic ions

C6H12O6

Molecular formula

Nitrogen

N3-

Nick the camel ate an inch clam for supper in phoenix

Nick= Nitrate (1 vowel= charge, 3 constants= #'s of oxygen) N1O3 (-1) Camel= Carbonate CO3 (2-) Clam= Chlorate ClO3 (1-) Supper= Sulfate SO4 (2-) Phoenix= Phosphate PO4 (3-)

NO3(-)

Nitrate

NO2(-)

Nitrite

Phosphorus

P3-

ClO4 (-)

Perchlorate

MnO4 (-)

Permanganate

O2 (2-)

Peroxide

PO4 (3-)

Phosphate

Sulfur

S2-

Polyatomic Cations

Use (ium) ending

How do you name formulas that contain water?

Use greek prefixes to indicate number of water molecules 1/2 = hemi 1 = mono 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deca


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