Combo with "AP Chem Cations and Anions" and 13 others

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Avogadro's Law

"Equal volumes of gases at the same temp and pressure have the same number of molecules!"

ammonium dichromate

(NH₄)₂Cr₂O₇

ammonium sulfide

(NH₄)₂S

formal charge=

(valence e-) - [(nonbonding e-) + (.5 bonding e-)]

Define chemical formula and give an example.

- A chemical formula is the representation of chemical substances using their chemical symbols and appropriate subscripts for the numbers of atoms. - A simmple formula is Ca(NO₃)₂ - This formula indicates a compound with one calcium atom, two nitrogen atoms, and six oxygen atoms.

Define a hydrate and give an example.

- A hydrate is a substance that contains a fixed number of water molecules. - The water molecules are written separately from the formula itself and connected to it with a dot in the center of the line between the chemical formula and the water molecules. - For example, cobalt(II) chloride hexahydrate is CoCl₂∙6H₂O.

Define metal.

- A metal is a substance with characteristic properties of high electrical conductivity, malleability, and a metallic-silver or yellow luster. - A metal can also be described as the nucleus and core electrons in a "sea of valence electrons."

Define metalloid.

- A metalloid is an element that has properties of both metals and nonmetals. - They are useful as semiconductors. - Examples are silicon and germanium, which are used for transistors and integrated circuits.

Define proton.

- A proton is one of the three particles that make up the atom along with an electron and a neutron. - The proton has a positive charge, equal in magnitude (but with the opposite sign) to the charge of the electron. - The number of protons is equal to the atomic number of an element. - Protons, along with neutrons, are located in the nucleus and make up the bulk of an atom's mass.

Describe the three states of matter.

- A solid retains both volume and shape and molecules are relatively rigid in a crystal lattice. - A liquid retains volume but not shape, molecules move freely in close contact, and strong attractive forces are present. - A gas assumes the volume and shape of a container, molecules are almost totally independent of each other, there is little in the way of attractive forces, and it is highly compressable.

What is an amorphous substance?

- Amorphous means without structure. - Amorphous substances have no long-range crystal structure. - Glass is an example of an amorphous substance.

Define electron, neutron and proton.

- An electron occupies space outside the nucleus. Mass = 0, charge = 1-, symbol is e- - A neutron is an uncharged particle in the nucleus. Symbol is ¹n, mass = 1 - A proton is positively charged article in the nucleus. Symbol is ¹₁p, mass =1, charge = 1+ Number of protons defines the identity of an atom

What concept includes allotropes?

- An element exhibits allotropy when it can exist as two or more distinct chemical structures. - For example: the three allotropes of carbon, graphite, diamond, and C₆₀(buckminsterfullerence). - Not all elements have allotropes.

Define ion.

- An ion is an element that has lost or gained one or more electrons. - A cation has lost one or more electrons. - An anion has gained one or more electrons. - A polyatomic ion is a group of elements bound together covalently that also carries a charge.

What is the concept behind a chemical compound?

- Chemists envision a chemical compound as a substance that has a fixed ratio (by either mass or atoms) of two or more different atoms. - Chemical compounds have definite physical properties that can be used to identify the compound. - Chemical compounds also have characteristic chemical properties that indicate what reactions they participate in and what reactions they do not.

Define electron configuration.

- Electron configuration is a listing of the electrons within an atom based upon the sublevels that are filled and relative energies of these sublevels. The electron configuration for silicon is 1s²2s²2p⁶3s²3p². - It is also the sequence in which the sublevel fills can be read, row by row, from the periodic table.

Define element.

- Element is the term given to any one of the 118 distinct particles of known atoms. - Each had distinct chemical and physical properties. - Elements are organized on the basis of atomic numbers in the periodic table.

Define malleable.

- Malleable is a property of metals. - Malleable means that the substance can be hammered into new shapes.

Define metallic crystal.

- Metallic crystals form from the metals in the periodic table. - These crystals are malleable, ductile, and conduct electricity. - Chemists view metallic crystals as a lattice of nuclei and core electrons in a "sea" of mobile valence electrons.

- Describe where on the periodic table metals, nonmetals, and metalloids are found. - Describe their properties.

- Metals are found on the lower left of the periodic table, nonmetals on the upper right of the table, and metalloids are on either side of a staircase line that starts between boron and aluminum, aluminum to silicon, and then to the bottom of the table. - Metals typically have a silvery luster (except gold and copper), conduct electricity easily, and are malleable and ductile. - Nonmetals have none of the properties that metals have. - Metalloids have properties in between metals and nonmetals. They are semiconductors of electricity.

Define noble gases.

- Noble gases are the elements in the last group in the periodic table (Group ViiiA or 18). - They are unusually stable elements and all, except He, have ns², np⁶ valence electrons. - The noble gases include: - helium, He - neon, Ne - argon, Ar - krypton, Kr - xenon, Xe - radon, Rn

Describe the nuclear charge and the concept of effective nuclear charge.

- Nuclear charge is the number of positive charges in the nucleus. This is the same as the number of protons in the nucleus (Z) and is also the atomic number. - The concept of effective nuclear charge is that inner (core) electrons shield outer electrons from the nuclear charge. The outer electrons are attracted by a nuclear that is approximately equal to the number of valence electrons. - The atomic radius decreases from left to right across the periodic table because the effective nuclear charge increases as the number of valence electrons increases. The increase in effective nuclear charge increases the attractive force on the valence electrons, resulting in a smaller atom.

Amphoteric and amphiprotic substances have the same underlying concept. Explain.

- Substances that can both donates and accept protons are amphiprotic. Example: H₂PO₄₋. - Substances that can react as both an acid and a base are amphoteric. Example: Al₂O₃.

Define Bohr atom.

- The Bohr atom is the model of the atom developed by Niels Bohr. - This model viewed electrons circling the nucleus like a miniature solar system. - Each orbit had a definite energy and electrons moving from one orbit to another and either absorbed or emitted the energy difference between the orbits. - This theory replicated the Rydberg Constant to less than +-0.5%.

What is the Pauli Exclusion Principle?

- The Pauli Exclusion Principle requires that no two electrons in an atom may have the same set of four quantum numbers: n, l, ml, and ms. - This is also means that no two electrons with the same wave equations can coexist. - Another interpretation is that no two electrons can occupy exactly the same space at the same time.

Define periodic table, period, and group.

- The arrangement of the elements in an orderly fashion that shows the relationships of their electronic, chemical, and physical characteristics is the modern periodic table. - Each row in the table is called a period. - Each column in the talbe is called a group (and sometimes family).

What is the concept behind the atomic number?

- The atomic number is the number that specifies the position of an element in the periodic table. - It is also a number representing the number of protons in the nucleus of an atom. - The atomic number defines the identity of an element. The basic ida is that each element must fall in some sort of order. Mendeleev originally based the order on atomic masses. It was later found that the order should be based on the number of protons in the nucleus of an element.

- What is the formula for aluminum fluoride? - What are the symbols for the ions that make up this compound?

- The formula for aluminum fluoride is AlF₃. - The ions that make up this compound are Al³⁺ and F⁻.

- What is the formula for aluminum hydrogen sulfate or aluminum bisulfate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for aluminum hydrogen sulfate is Al(HSO₄)₃. - The ions that make up this compound are Al³⁺ and HSO₄⁻. - The oxidation number of S is +6. - The HSO₄⁻ ion is often called the bisulfate ion.

- What is the formula for aluminum nitrate nonahydrate? - What are the symbols for the ions that make up this compound?

- The formula for aluminum nitrate nonahydrate is Al(NO₃)₃∙9H₂O. - The ions that make up this compound are Al³⁺ and NO₃⁻.

- What is the formula for aluminum sulfate? - What are the symbols for the ions that make up this compound?

- The formula for aluminum sulfate is Al₂(SO₄)₃. - The ions that make up this compound are Al³⁺ and SO₄²⁻.

- What is the formula for ammonium nitrate (fertilizer)? - What are the symbols for the ions that make up this compound?

- The formula for ammonium nitrate is NH₄NO₃. - The ions that make up this compound are NH₄⁺ and NO₃⁻.

- What is the formula for ammonium sulfate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nitrogen in the ammonium ion?

- The formula for ammonium sulfate is (NH₄)₂SO₄. - The ions that make up this compound are NH₄⁺ and SO₄²⁻. - The oxidation number of N is -3.

- What is the formula for ammonium sulfite? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for ammonium sulfite is (NH₄)₂SO₃. - The ions that make up this compound are NH₄⁺ and SO₃²⁻. - The oxidation number of S is +4.

- What is the formula for barium hydroxide octahydrate? - What are the symbols for the ions that make up this compound?

- The formula for barium hydroxide octahydrate is Ba(OH)₂∙8H₂O. - The ions that make up this compound are Ba²⁺ and OH⁻.

- What is the formula for calcium bromate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for calcium bromate is Ca(BrO₃)₂. - The ions that make up this compound are Ca²⁺ and BrO₃⁻. - The oxidation number of Br is +5.

- What is the formula for calcium carbonate (limestone)? - What are the symbols for the ions that make up this compound?

- The formula for calcium carbonate is CaCO₃. - The ions that make up this compound are Ca²⁺ and CO₃²⁻.

- What is the formula for calcium chlorate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for calcium chlorate is Ca(ClO₃)₂. - The ions that make up this compound are Ca²⁺ and ClO₃⁻. - The oxidation number of Cl is +5.

- What is the formula for calcium chloride dihydrate? - What are the symbols for the ions that make up this compound?

- The formula for calcium chloride dihydrate is CaCl₂∙2H₂O. - The ions that make up this compound are Ca²⁺ and Cl⁻.

- What is the formula for calcium hydrogen sulfite? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for calcium hydrogen sulfite is Ca(HSO₃)₂. - The ions that make up this compound are Ca²⁺ and HSO₃⁻. - The oxidation number of S is +4.

- What is the formula for calcium nitride? - What are the symbols for the ions that make up this compound?

- The formula for calcium nitrde is Ca₃N₂. - The ions that make up this compound are Ca²⁺ and N³⁻.

- What is the formula for calcium oxide (lime)? - What are the symbols for the ions that make up this compound?

- The formula for calcium oxide is CaO. - The ions that make up this compound are Ca²⁺ and O²⁻.

- What is the formula for calcium sulfate (plaster of Paris)? - What are the symbols for the ions that make up this compound?

- The formula for calcium sulfate is CaSO₄. - The ions that make up this compound are Ca²⁺ and SO₄²⁻.

- What is the formula for chromium(III) phosphate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for chromium(III) phosphate is CrPO₄. - The ions that make up this compound are Cr³⁺ and PO₄³⁻. - The oxidation number of P is +5.

- What is the formula for chromium(III) sulfite? - What are the symbols for the ions that make up this compound?

- The formula for chromium(III) sulfite is Cr₂(SO₃)₃. - The ions that make up this compound are Cr³⁺ and SO₃²⁻.

- What is the formula for cobalt(III) chloride? - What are the symbols for the ions that make up this compound?

- The formula for cobalt(III) chloride is CoCl₃. - The ions that make up this compound are Co³⁺ and Cl⁻.

- What is the formula for copper sulfate pentahydrate? - What are the symbols for the ions that make up this compound?

- The formula for copper sulfate pentahydrate is CuSO₄∙5H₂O. - The ions that make up this compound are Cu²⁺ and SO₄²⁻.

- What is the formula for gold(III) phosphate? - What are the symbols for the ions that make up this compound?

- The formula for gold(III) phosphate is AuPO₄. - The ions that make up this compound are Au³⁺ and PO₄³⁻.

- What is the formula for iron(III) nitrate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for iron(III) nitrate is Fe(NO₃)₃. - The ions that make up this compound are Fe³⁺ and NO₃⁻. - The oxidation number of N is +5.

- What is the formula for lead(II) acetate? - What are the symbols for the ions that make up this compound?

- The formula for lead(II) acetate is Pb(C₂H₃O₂)₂. - The ions that make up this compound are Pb²⁺ and C₂H₃O₂⁻.

- What is the formula for lead(IV) phosphate? - What are the symbols for the ions that make up this compound?

- The formula for lead(IV) phosphate is Pb₃(PO₄)₄. - The ions that make up this compound are Pb⁴⁺ and PO₄³⁻.

- What is the formula for lithium bromide? - What are the symbols for the ions that make up this compound?

- The formula for lithium bromide is LiBr. - The ions that make up this compound are Li⁺ and Br⁻.

- What is the formula for lithium bromite? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for lithium bromite is LiBrO₂. - The ions that make up this compound are Li⁺ and BrO₂⁻. - The oxidation number of Br is +3.

- What is the formula for lithium carbonate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for lithium carbonate is Li₂CO₃. - The ions that make up this compound are Li⁺ and CO₃²⁻. - The oxidation number of C is +4.

- What is the formula for magnesium chloride hexahydrate? - What are the symbols for the ions that make up this compound?

- The formula for magnesium chloride hexahydrate is MgCl₂∙6H₂O. - The ions that make up this compound are Mg²⁺ and Cl⁻.

- What is the formula for magnesium hydroxide? - What are the symbols for the ions that make up this compound?

- The formula for magnesium hydroxide is Mg(OH)₂. - The ions that make up this compound are Mg²⁺ and OH⁻.

- What is the formula for magnesium phosphide? - What are the symbols for the ions that make up this compound?

- The formula for magnesium phosphide is Mg₃P₂. - The ions that make up this compound are Mg²⁺ and P³⁻.

- What is the formula for mercury(I) iodide? - What are the symbols for the ions that make up this compound?

- The formula for mercury(I) iodide is Hg₂I₂. - The ions that make up this compound are Hg₂²⁺ and I⁻.

- What is the formula for nickel(II) hydrogen carbonate or nickel(II) bicarbonate? - What are the symbols for the ions that make up this compound?

- The formula for nickel(II) hydrogen carbonate is Ni(HCO₃)₂. - The ions that make up this compound are Ni²⁺ and HCO₃⁻. The HCO₃⁻ ion is also called bicarbonate.

- What is the formula for potassium dichromate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for potassium dichromate is K₂Cr₂O₇. - The ions that make up this compound are K⁺ and Cr₂O₇²⁻. - The oxidation number of Cr is +6.

- What is the formula for potassium dihydrogen phosphate? - What are the symbols for the ions that make up this compound?

- The formula for potassium dihydrogen phosphate is KH₂PO₄. - The ions that make up this compound are K⁺ and H₂PO₄⁻.

- What is the formula for potassium permanganate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for potassium permanganate is KMnO₄. - The ions that make up this compound are K⁺ and MnO₄⁻. - The oxidation number of Mn is +7.

- What is the formula for rubidium perbromate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for rubidium perbromate is RbBrO₄. - The ions that make up this compound are Rb⁺ and BrO₄⁻. - The oxidation number of Br is +7.

- What is the formula for silver chloride? - What are the symbols for the ions that make up this compound?

- The formula for silver chloride is AgCl. - The ions that make up this compound are Ag⁺ and Cl⁻.

- What is the formula for silver chromate? - What are the symbols for the ions that make up this compound?

- The formula for silver chromate is AgCrO₄. - The ions that make up this compound are Ag⁺ and CrO₄²⁻.

- What is the formula for sodium chloride? - What are the symbols for the ions that make up this compound?

- The formula for sodium chloride is NaCl. - The ions that make up this compound are Na⁺ and Cl⁻.

- What is the formula for sodium chromate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for sodium chromate is Na₂CrO₄. - The ions that make up this compound are Na⁺ and CrO₄²⁻. - The oxidation number of Cr is +6.

- What is the formula for sodium hydrogen phosphate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for sodium hydrogen phosphate is Na₂HPO₄. - The ions that make up this compound are Na⁺ and HPO₄²⁻. - The oxidation number of P is +5.

- What is the formula for sodium hypobromite? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for sodium hypobromite is NaBrO. - The ions that make up this compound are Na⁺ and BrO⁻. - The oxidation number of Br is +1.

- What is the formula for sodium hypochlorite? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for sodium hypochlorite is NaClO. - The ions that make up this compound are Na⁺ and ClO⁻. - The oxidation number of Cl is +1.

- What is the formula for sodium nitrite (food preservative)? - What are the symbols for the ions that make up this compound?

- The formula for sodium nitrite is NaNO₂. - The ions that make up this compound are Na⁺ and NO₂⁻.

- What is the formula for sodium nitrite? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for sodium nitrite is NaNO₂. - The ions that make up this compound are Na⁺ and NO₂⁻. - The oxidation number of N is +3.

- What is the formula for sodium oxalate? - What are the symbols for the ions that make up this compound?

- The formula for sodium oxalate is Na₂C₂O₄. - The ions that make up this compound are Na⁺ and C₂O₄²⁻.

- What is the formula for sodium oxide? - What are the symbols for the ions that make up this compound?

- The formula for sodium oxide is Na₂O. - The ions that make up this compound are Na⁺ and O²⁻.

- What is the formula for strontium iodide? - What are the symbols for the ions that make up this compound?

- The formula for strontium iodide is SrI₂. - The ions that make up this compound are Sr²⁺ and I⁻.

- What is the formula for tin(II) carbonate? - What are the symbols for the ions that make up this compound?

- The formula for tin(II) carbonate is SnCO₃. - The ions that make up this compound are Sn²⁺ and CO₃²⁻.

- What is the formula for titanium(II) chlorite? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for titanium(II) chlorite is Ti(Clo₂)₂. - The ions that make up this compound are Ti²⁺ and ClO₂⁻. - The oxidation number of Cl is +3.

- What is the formula for tungsten(VI) oxide? - What are the symbols for the ions that make up this compound?

- The formula for tungsten(VI) oxide is WO₃. - The ions that make up this compound are W⁶⁺ and O²⁻.

- What is the formula for zinc sulfate? - What are the symbols for the ions that make up this compound? - What is the oxidation number of the nonoxygen element in the polyatomic ion?

- The formula for zinc sulfate is ZnSO₄. - The ions that make up this compound are Zn²⁺ and SO₄²⁻. - The oxidation number of S is +6.

Define nucleus.

- The nucleus is the center of the atom that contains the protons and neutrons. - It comprises an extremely small fraction of the atom's volume. - The nucleus is extremely dense while the rest of the atom is primarily empty space.

Define and describe the four quantum numbers.

- The principal quantum number, n, indicates the shell (or principal energy level) of the atom min which and electron resides and is a rough measure of the distance from the nucleus. n can have any value from 1 to infinity. - The azimuthal quantum number, l, specifies the sublevel (or orbital) that an electron is located in. This number may be any number from zero up to n-1. This number specifies the shape of an atomic orbital. - The magnetic quantum number,m, indicates the orientation of a sublevel in space. The value of the m, quantum number can be any number from -l to zero to +l. - The spin quantum number,ms, indicates the spin of the electron. An electron is not actually spinning but it is a useful way of visualizing this property. Acceptable values for spin are +¹/₂ and -¹/₂. - Each electron possesses four quantum numbers. Each electron in an atom must have a set of four quantum numbers different from all other electrons in that atom.

What are the subatomic constituents of the atom?

- The subatomic constituents of the atom are protons and neutrons in the nucleus and electrons around the nucleus. - The atomic number Z=# of protons. - The mass number A=# protons + # of neutrons.

Define transition elements and inner transition elements.

- Transition elements are sometimes called d-block elements because the last electrons added to form the element are electrons occupying d orbitals. -They occupy the 10 groups in the center of the periodic table. -They often form colored ionic compounds. -They often have multiple possible oxidation states. -They often form polyatomic anions. - Inner transition elements have electrons occupying f orbitals as the last electrons added to their electron configuration. -They occupy the 14 groups that are often placed outside the periodic table. -They contain many of the radioactive and manmade elements.

Define weight and mass.

- Weight is the force developed due to the gravitational attraction of two masses toward each other. The weight of an object changes as the gravitational acceleration changes. weight=force=mass X acceleration of gravity - Mass is the amount of material in a sample. Mass does not change with the acceleration of gravity.

colligative properties - examples

- vapor pressure lowering - freezing point depression - boiling point elevation - osmotic pressure

changes in temperature (le chat)

1. exothermic: shifts left (rcnts > prod + heat) 2. endothermic: shifts right (heat + rcnts > prod)

changes in pressure/volume (le chat)

1. increase volume, decrease pressure, reaction shifts to side with more moles. 2. decrease volumes, increase pressure, reaction shifts to side with lesser moles. 3. if moles are equal, no shift occurs.

Entropy increases when:

1. molecules increase 2. temp increases 3. l - g, s- g, s - l

left to right

1. radius decreases 2. ionization energy, electronegativity, and electron affinity increase

top to bottom

1. radius increases 2. ionization energy, electronegativity, and electron affinity decrease

D

2 K + 2 H2O ---> 2 K+ + 2 OH¯ + H2 When 0.400 mole of potassium reacts with excess water at standard temperature and pressure as shown in the equation above, the volume of hydrogen gas produced is (A) 1.12 liters (B) 2.24 liters (C) 3.36 liters (D) 4.48 liters (E) 6.72 liters

E

6 I¯ + 2 MnO4¯ + 4 H2O(l) ---> 3 I2(s) + 2 MnO2(s) + OH¯ Which of the following statements regarding the reaction represented by the equation above is correct? (A) Iodide ion is oxidized by hydroxide ion. (B) MnO4¯ is oxidized by iodide ion. (C) The oxidation number of manganese changes from +7 to +2. (D) The oxidation number of manganese remains the same. (E) The oxidation number of iodine changes from -1 to 0.

G = 0

@ equilibrium

C

A 1.0 L sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl2. What is the minimum number of moles of AgNO3 that must be added to the solution in order to precipitate all of the Cl¯ as AgCl(s) ? (Assume that AgCl is insoluble.) (A) 0.10 mol (B) 0.20 mol (C) 0.30 mol (D) 0.40 mol (E) 0.60 mol

C

A 2.00-liter sample of nitrogen gas at 27 °C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is (A) 68 °C (B) 120 °C (C) 477 °C (D) 677 °C (E) 950. °C

C

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.50 mole of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen? (A) 0.13 atm (B) 0.27 atm (C) 0.63 atm (D) 0.90 atm (E) 6.3 atm

E

A hot-air balloon rises. Which of the following is the best explanation for this observation? (A) The pressure on the walls of the balloon increases with increasing tempearature. (B) The difference in temperature between the air inside and outside the ballon produces convection currents. (C) The cooler air outside the balloon pushes in on the walls of the ballon. (D) The rate of diffusion of cooler air is less than that of warmer air. (E) The air density inside the ballon is less than that of the surrounding air.

C

A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0 °C and 1.00 atmosphere. A possible formula for the hydrocarbon is (A) CH2 (B) C2H4 (C) C3H6 (D) C4H8 (E) C5H10

D

A measured mass of an unreactive metal was dropped into a small graduated cylinder half filled with water. The following measurements were made. Mass of metal = 19.611 grams Volume of water before addition of metal = 12.4 milliliters Volume of water after addition of metal = 14.9 milliliters The density of the metal should be reported as (A) 7.8444 grams per mL (B) 7.844 grams per mL (C) 7.84 grams per mL (D) 7.8 grams per mL (E) 8 grams per mL

anion

A negatively charged ion

cation

A positively charged ion

C

A sample of 0.0100 mole of oxygen gas is confined at 37° C and 0.216 atmosphere. What would be the pressure of this sample at 15° C and the same volume? (A) 0.0876 atm (B) 0.175 atm (C) 0.201 atm (D) 0.233 atm (E) 0.533 atm

D

A sample of 3.30 grams of an ideal gas at 150.0 °C and 1.25 atmospheres pressure has a volume of 2.00 liters. What is the molar mass of the gas? The gas constant, R, is 0.0821 L atm mol¯1 K¯1). (A) 0.0218 gram/mole (B) 16.2 grams/mole (C) 37.0 grams/mole (D) 45.8 grams/mole (E) 71.6 grams/mole

C

A sample of 61.8 g of H3BO3, a weak acid is dissolved in 1,000 g of water to make a 1.0-molal solution. Which of the following would be the best procedure to determine to molarity of the solution? (Assume no additional information is available.) (A) Titration of the solution with standard acid (B) Measurement of the pH with a pH meter (C) Determination of the boiling point of the solution (D) Measurement of the total volume of the solution (E) Measurement of the specific heat of the solution

C

A sample of an ideal gas is cooled from 50.0 °C to 25.0 °C in a sealed container of constant volume. Which of the following values for the gas will decrease? I. The average molecular mass of the gas II. The average distance between the molecules III. The average speed of the molecules (A) I only (B) II only (C) III only (D) I and III (E) II and III

E

A solution is known to contain an inorganic salt of one of the following elements. The solution is colorless. The solution contains a salt of (A) Cu (B) Mn (C) Fe (D) Ni (E) Zn

A

A white solid is observed to be insoluble in water, insoluble in excess ammonia solution, and soluble in dilute HCl. Which of the following compounds could the solid be? (A) CaCO3 (B) BaSO4 (C) Pb(NO3)2 (D) AgCl (E) Zn(OH)2

A

A yellow precipitate forms when 0.5 M NaI(aq) is added to a 0.5 M solution of which of the following ions? A) Pb2+(aq) B) Zn2+(aq) C) CrO42¯(aq) D) SO42¯(aq) E) OH¯(aq)

C₂H₃O₂⁻¹

Acetate

A

Adding water to some chemicals can be dangerous because large amounts of heat are liberated. Which of the following does NOT liberate heat when water is added to it? (A) KNO3 (B) NaOH (C) CaO (D) H2SO4 (E) Na

B

After completing an experiment to determine gravimetrically the percentage of water in a hydrate, a student reported a value of 38 percent. The correct value for the percentage of water in the hydrate is 51 percent. Which of the following is the most likely explanation for this difference? A) Strong initial heating caused some of the hydrate sample to spatter out of the crucible. B) The dehydrated sample absorbed moisture after heating. C) The amount of the hydrate sample used was too small. D) The crucible was not heated to constant mass before use. E) Excess heating caused the dehydrated sample to decompose.

Silver

Ag

Silver

Ag +1

silver nitrite

AgNO₂

Aluminum

Al

Aluminum

Al +3

aluminum hydroxide

Al(OH)₃

aluminum selenide

Al2Se3

aluminum fluoride

AlF₃

Define alkali metals

Alkali metals are the elements in the first group (column) of the periodic table (IA or 1). All: - have ns¹ electrons as valance electrons - are extremely reactive elements - have low ionization energies - have low electronegativities - are metals that form 1+ ions

Define alkaline earth metals.

Alkaline earth metals are the elements in the second group (column) of the periodic table. All: - have ns² electrons for valence electrons - are very reactive elements - are metals that form 2+ ions

Al⁺³

Aluminum

aluminum chromate

Al₂(CrO₄)₃

NH₂⁻¹

Amide

NH₄⁺¹

Ammonium

C

An impossible electronic configuration (A) 1s2 2s2 2p5 3s2 3p5 (B) 1s2 2s2 2p6 3s2 3p6 (C) 1s2 2s2 2p6 2d10 3s2 3p6 (D) 1s2 2s2 2p6 3s2 3p6 3d5 (E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2

Define isotope.

An isotope is an atom with a specific number of neutrons in addition to the protons and electrons defined by the atomic number. A given element may have several isotopes, each of which has a different number of neutrons while having he same number of electrons and protons. - For example: C-12, C-13, and C-14. Each has 6 electrons and 6 protons; however, they have 6,7, and 8 neutrons, respectively.

Sb⁺³

Antimony (III) or Antiminous

Sb⁺⁵

Antimony (V) or Antimonic

Argon

Ar

AsO₄⁻²

Arsenate

As⁻³

Arsenide

Arsenic

As

C

As the temperature is raised from 20 ° C to 40 ° C, the average kinetic energy of neon atoms changes by a factor of (A) 1/2 (B) [square root of](313/293) (C) 313/293 (D) 2 (E) 4

Arsenate

AsO4 -3

Astatine

At

D

At 25 °C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050 mole per minute. Under the same conditions, which of the following gases effuses at approximately one-half that rate? (A) O2 (molar mass 32 grams) (B) He2 (molar mass 4.0 grams) (C) CO2 (molar mass 44 grams) (D) Cl2 (molar mass 71 grams) (E) CH4 (molar mass 16 grams)

Gold

Au

Gold

Au +1 and +3

Boron

B

Borate

BO3 -3

Barium

Ba

barium hypochlorite

Ba(ClO)₂

barium hydroxide

Ba(OH)₂

barium oxide

BaO

Ba⁺²

Barium

Beryllium

Be

Be⁺²

Beryllium

Bismuth

Bi

BO₃⁻³

Borate

B⁺³

Boron

Bromine

Br

HypoBromite

BrO -1

Bromate

BrO3 -1

bromate

BrO₃⁻

BrO₃⁻¹

Bromate

Br⁻¹

Bromide

BrO₂⁻¹

Bromite

Carbon

C

Acetate

C2H3O2 -1

Oxalate

C2O4 -2

Tartrate

C4H4O6 -2

C

CCl4, CO2, PCl3, PCl5, SF6 Which of the following does not describe any of the molecules above? (A) Linear (B) Octahedral (C) Square planar (D) Tetrahedral (E) Trigonal pyramidal

D

CH3CH2OH boils at 78 °C and CH3OCH3 boils at - 24 °C, although both compounds have the same composition. This difference in boiling points may be attributed to a difference in (A) molecular mass (B) density (C) specific heat (D) hydrogen bonding (E) heat of combustion

methane

CH₄

Cyanide

CN -1

cyanide

CN⁻

Carbonate

CO3 -2

carbonate

CO₃²⁻

Calcium

Ca

calcium chlorite

Ca(ClO₂)₂

calcium oxide

CaO

Cd⁺²

Cadmium

Ca⁺²

Calcium

C

Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter

C⁻⁴

Carbide

D

Carbon dioxide, CO2(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

CO₃⁻²

Carbonate

calcium phosphate

Ca₃(PO₄)₂

Cadmium

Cd

cadmium selenide

CdSe

Cs⁺¹

Cesium

A

Cesium chloride, CsCl (s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

ClO₃⁻¹

Chlorate

Cl⁻¹

Chloride

ClO₂⁻¹

Chlorite

CrO₄⁻²

Chromate

Cr⁺²

Chromium (II) or Chromous

Cr⁺³

Chromium (III) or Chromic

Chlorine

Cl

Hypochlorite

ClO -1

Chlorite

ClO2 -1

Chlorate

ClO3 -1

Perchlorate

ClO4 -1

hypochlorite

ClO⁻

chlorite

ClO₂⁻

chlorate

ClO₃⁻

perchlorate

ClO₄⁻

dichlorine heptoxide

Cl₂O₇

Cobalt

Co

Cobalt

Co +2 and +3

cobalt (III) nitrate

Co(NO3)3

Co⁺²

Cobalt(II) or Cobaltous

Co⁺³

Cobalt(III) or Cobaltic

C

Contains 1 sigma (s) and 2 pi (p) bonds (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2

Cu⁺¹

Copper(I) or Cuprous

Cu⁺²

Copper(II) or Cupric

Chromium

Cr

Chromium

Cr +2 and +3

chromium(III) nitrate

Cr(NO₃)₃

chromium (II) carbonate

Cr2(CO3)3

DiChromate

Cr2O7 -2

Chromate

CrO4 -2

chromate

CrO₄²⁻

dichromate

Cr₂O₇²⁻

Cesium

Cs

Copper

Cu

Copper

Cu +1 and +2

copper (II) bicarbonate

Cu(HCO₃)₂

copper (II) nitrate

Cu(NO3)2

copper(II) bromide

CuBr₂

copper (I) chloride

CuCl

copper(I) selenide

Cu₂Se

CN⁻¹

Cyanide

acetate

C₂H₃O₂⁻

ethene

C₂H₄

ethane

C₂H₆

oxalate

C₂O₄²⁻

pentane

C₅H₁₂

Colligative Properties

Depend on the amount of solute particles

Cr₂O₇⁻²

Dichromate

H₂PO₄⁻¹

Dihydrogen phosphate

Positive deviation of Raoult's Law

Endothermic reaction. Weak interactions between solute and solvent. Higher tendency to escape into gas phase.

A

Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel at room temperature. If the vessel has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial pressures of the gases remaining in the vessel after some of the gas mixture has effused? A) PHe < PNe < PAr B) PHe < PAr < PNe C) PNe < PAr < PHe D) PAr < PHe < PNe E) PHe = PAr = PNe

CH3-CH2-CH2-CH3 and CH (with 3 CH3 attached w/ a single bond)

Examples of isomers

Negative deviation of Raoult's Law

Exothermic reactions. Strong interaction between solute and solvent. Lower tendency to escape into gas phase

E

Explains the experimental phenomenon of electron diffraction (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter

Fluorine

F

Iron

Fe

Iron

Fe +2 and +3

iron(II) cyanide

Fe(CN)₂

iron(II) sulfide

FeS

FO₃⁻¹

Fluorate

F⁻¹

Fluoride

FO₂⁻¹

Fluorite

D

For the substance represented in the diagram, which of the phases is most dense and which is least dense at - 15 °C. Most Dense Least Dense (A) Solid Gas (B) Solid Liquid (C) Liquid Solid (D) Liquid Gas (E) The diagram gives no information about densities.

Francium

Fr

The frequency of a photon is____________ to its wavelength. a. directly proportional b. inversely proportional c. not related If a or b is chose, write the appropriate equation.

Frequency is inversely proportional to wavelength, as shown in the equation: v(frequency)=c

Gallium

Ga

gallium arsenide

GaAs

Germanium

Ge

Au⁺¹

Gold

B

Gold, Au(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

Hydrogen

H

D

H2(g) + (1/2) O2(g) ---> H2O(l) DH° = - 286 kJ 2 Na(s) + (1/2) O2(g) ---> Na2O(s) DH° = - 414 kJ Na(s) + (1/2) O2(g) + (1/2) H2(g) ---> NaOH(s) DH° = - 425 kJ Based on the information above, what is the standard enthalpy change for the following reaction? Na2O(s) + H2O(l) ---> 2 NaOH(s) (A) -1,125 kJ (B) -978 kJ (C) -722 kJ (D) -150 kJ (E) +275 kJ

Dihydrogen phosphate

H2PO4 -1

hydrobromic acid

HBr

Hydrogen carbonate

HCO3 -1

hydrogen carbonate (bicarbonate)

HCO₃⁻

hydrochloric acid

HCl

perchloric acid

HClO₄

acetic acid

HC₂H₃O₂

iodous acid

HIO2

nitrous acid

HNO2

Hydrogen Phospate

HPO4 -2

Hydrogen Sulfide

HS -1

Hydrogen Sulfite

HSO3 -1

hydrogen sulfite (bisulfite)

HSO₃⁻

hydrogen sulfate (bisulfate)

HSO₄⁻

Define halogen.

Halogens are the elements in the next to last group of the periodic table (Group VIIA or 17). They are reactive elements with an ns², np⁵ valence electron structure. - Halogens commonly form salts (halide is another name for salt) with metals. - Halogens generally have high electronegativities. Fluorine has the highest electronegativity in the periodic table. - In simple compounds, halogens tend to form only one bond. However, halogens form multiple bonds with oxygen and other halogens.

D

Has a bond order of 2 (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2

C

Has the largest bond-dissociation energy (A) Li2 (B) B2 (C) N2 (D) O2 (E) F2

Helium

He

Mercury

Hg

Mercury

Hg +2

mercury (I) chloride

Hg2Cl2 (mercury exists as Hg2 2+ ions)

mercury (I) chloride

Hg₂Cl₂

E

How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen atoms? (A) 164 grams (B) 96 grams (C) 62 grams (D) 50. grams (E) 41 grams

C

How many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0-molar HCl? (A) 3.9 mL (B) 35 mL (C) 260 mL (D) 1,000 mL (E) 3,900 mL

A

How many moles of solid Ba(NO3)2 should be added to 300. milliliters of 0.20-molar Fe(NO3)3 to increase the concentration of the NO3¯ ion to 1.0-molar? (Assume that the volume of the solution remains constant.) (A) 0.060 mole (B) 0.12 mole (C) 0.24 mole (D) 0.30 mole (E) 0.40 mole

Define Hund's Rule.

Hund's Rule states that all orbitals in a sublevel must fill with one electron before a second electron of opposite spin can be added to any orbital in that sublevel.

H⁻¹

Hydride

H⁺¹

Hydrogen

HSO₃⁻¹

Hydrogen Sulfite or Bisulfite

HCO₃⁻¹

Hydrogen carbonate or Bicarbonate

B

Hydrogen gas is collected over water at 24 °C. The total pressure of the sample is 755 millimeters of mercury. At 24 °C, the vapor pressure of water is 22 millimeters of mercury. What is the partial pressure of the hydrogen gas? (A) 22 mm Hg (B) 733 mm Hg (C) 755 mm Hg (D) 760 mm Hg (E) 777 mm Hg

HPO₄⁻²

Hydrogen phosphate

HSO₄⁻¹

Hydrogen sulfate or bisulfate

OH⁻¹

Hydroxide

BrO⁻¹

Hypobromite

ClO⁻¹

Hypochlorite

FO⁻¹

Hypofluorite

IO⁻¹

Hypoiodite

carbonic acid

H₂CO₃

chromic acid

H₂CrO₄

dihydrogen monoxide

H₂O

dihydrogen phosphate

H₂PO₄⁻

sulfurous acid

H₂SO₃

phosphoric acid

H₃PO₄

Iodine

I

B

I2(g) + 3 Cl2(g) ---> 2 ICl3(g) According to the data in the table below, what is the value of DH° for the reaction represented above? Bond Average Bond Energy (KJ/mole) I---I 149 Cl---Cl 239 I---Cl 208 (A) - 860 kJ (B) - 382 kJ (C) + 180 kJ (D) + 450 kJ (E) + 1,248 kJ

HypoIodite

IO -1

Iodate

IO3 -1

Periodate

IO4 -1

iodine dioxide

IO₂

iodate

IO₃⁻

E

If 87 grams of K2 SO4 (molar mass 174 grams) is dissolved in enough water to make 250 milliliters of solution, what are the concentrations of the potassium and the sulfate ions? [K+] [SO42¯] (A) 0.020 M 0.020 M (B) 1.0 M 2.0 M (C) 2.0 M 1.0 M (D) 2.0 M 2.0 M (E) 4.0 M 2.0 M

Tyndall Effect

If it is a colloid, the light will be reflected; if it is a homogeneous mixture the light will be invisible

Indium

In

E

In a molecule in which the central atom exhibits sp3d2 hybrid orbitals, the electron pairs are directed toward the corners of (A) a tetrahedron (B) a square-based pyramid (C) a trigonal bipyramid (D) a square (E) an octahedron

B

In a qualitative ananlysis for the presence of Pb2+, Fe2+, and Cu2+ ions in a aqueous solution, which of the following will allow the separation of Pb2+ from the other ions at room temperature? A) Adding dilute Na2S(aq) solution B) Adding dilute HCl(aq) solution C) Adding dilute NaOH(aq) solution D) Adding dilute NH3(aq) solution E) Adding dilute HNO3(aq) solution

D

In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic radius? (A) It remains constant. (B) It increases only. (C) It increases, then decreases. (D) It decreases only. (E) It decreases, then increases.

B

In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.62 to 1.00 ? (A) CrO3 (B) CrO2 (C) CrO (D) Cr2O (E) Cr2O3

B

Indicates that an atomic orbital can hold no more than two electrons (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter

IO₃⁻¹

Iodate

I⁻¹

Iodide

IO₂⁻¹

Iodite

Iridium

Ir

Fe⁺²

Iron(II) or Ferrous

Fe⁺³

Iron(III) or Ferric

D

Is added to silicon to enhance its properties as a semiconductor (A) Pb (B) Ca (C) Zn (D) As (E) Na

D

Is used to explain the fact that the carbon-to-carbon bonds in benzene, C6H6, are identical (A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces)

B

Is used to explain the fact that the four bonds in methane are equivalent (A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces)

E

Is used to explain why iodine molecules are held together in the solid state (A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces)

A

Is used to explain why the boiling point of HF is greater than the boiling point of HBr (A) hydrogen bonding (B) hybridization (C) ionic bonding (D) resonance (E) van der Waals forces (London dispersion forces)

Potassium

K

potassium nitride

K3N

potassium cyanide

KCN

potassium chloride

KCl

potassium chlorate

KClO3

potassium permanganate

KMnO₄

Krypton

Kr

Lanthanum

La

Pb⁺²

Lead(II) or Plumbous

Pb⁺⁴

Lead(IV) or Plumbic

Lithium

Li

lithium nitride

Li3N

lithium hydrogen carbonate

LiHCO₃

Li⁺¹

Lithium

Molar Mass of a Gas

MM=dRT/P (Molar Mass = "dirty pee")

Mg⁺²

Magnesium

Mn⁺²

Manganese (II) or Manganous

Mn⁺³

Manganese (III) or Manganic

D

Mass of an empty container = 3.0 grams Mass of the container plus the solid sample = 25.0 grams Volume of the solid sample = 11.0 cubic centimeters The data above were gathered in order to determinethe density of an unknown solid. The density of the sample should be reported as (A) 0.5 g/cm3 (B) 0.50 g/cm3 (C) 2.0 g/cm3 (D) 2.00 g/cm3 (E) 2.27 g/cm3

Mass Percentage

Mass solute/Total Mass Solution

Hg₂⁺²

Mercury(I) or Mercurous

Hg⁺²

Mercury(II) or Mercuric

C

Methane, CH4(s) (A) Lattice of positive and negative ions held together by electrostatic forces. (B) Closely packed lattice with delocalized electrons throughout (C) Strong single covalent bonds with weak intermolecular forces. (D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces (E) Macromolecules held tgether with strong polar bonds.

Magnesium

Mg

magnesium phosphide

Mg3P2

Manganese

Mn

Manganese

Mn +2 and +3

Permanganate

MnO4 -1

permanganate

MnO₄⁻

Molybdenum

Mo

A

Molecules that have planar configurations include which of the following? I. BCl3 II. CHCl3 III. NCl3 (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III

Molarity

Moles solute/ Liter solution

molality

Moles solute/Kg solvent

Nitrogen

N

nitrogen trichloride

NCl₃

Ammonium

NH4 +1

ammonium acetate

NH4C2H3O2

ammonium hydrogen sulfate

NH4HSO4

ammonia

NH₃

ammonium

NH₄⁺

Nitrite

NO2 -1

Nitrate

NO3 -1

nitrite

NO₂⁻

nitrate

NO₃⁻

Sodium

Na

sodium oxide

Na2O

sodium peroxide

Na2O2

sodium hydride

NaH

sodium dihydrogen phosphate

NaH2PO4

sodium peroxide

Na₂O₂

Neon

Ne

Nickel

Ni

Nickle

Ni +2

Ni⁺²

Nickel (II) or Nickelous

Ni⁺³

Nickel (III) or Nickelic

NO₃⁻¹

Nitrate

N⁻³

Nitride

NO₂⁻¹

Nitrite

Define noble gas.

Noble gases are in the last group of the periodic table (Group VIIIA or 18). - They are unusually unreactive with an octet of valence electrons ns²np⁶. - Helium was first found in the sun's spectrum. - Xenon was the first noble gas that was made into a compound.

The van't Hoff factor is 1 for?

Nonelectrolytes, Not ionic

Neptunium

Np

dinitrogen tetrahydride

N₂H₄

dinitrogen trioxide

N₂O₃

Oxygen

O

E

O || CH3-C-CH2-CH3 The organic compound represented above is an example of (A) an organic acid (B) an alcohol (C) an ether (D) an aldehyde (E) a ketone

Peroxide

O2 -2

Hydroxide

OH -1

hydroxide

OH⁻

D

Of the following molecules, which has the largest dipole moment? (A) CO (B) CO2 (C) O2 (D) HF (E) F2

C

On a mountaintop, it is observed that water boils at 90°C, not at 100°C as at sea level. This phenomenon occurs because on the mountaintop the A) equilibrium water vapor pressure is higher due to the higher atmospheric pressure B) equilibrium water vapor pressure is lower due to the higher atmospheric pressure C) equilibrium water vapor pressure equals the atmospheric pressure at a lower temperature D) water molecules have a higher average kinetic energy due to the lower atmospheric pressure E) water contains a greater concentration of dissolved gases

C₂O₄⁻²

Oxalate

O⁻²

Oxide

Phosphorus

P

Gay-Lussac's Law

P/T = k P₁/T₁ = P₂/T₂

diphosphorus pentoxide

P2O5

PyroPhosphate

P2O7

phosphorus pentachloride

PCl₅

Phosphite

PO3 -3

Phosphate

PO4 -3

phosphite

PO₃³⁻

phosphate

PO₄³⁻

Boyle's Law

PV = k P₁V₁ = P₂V₂

Ideal Gas Law

PV=nRT

Lead

Pb

Lead

Pb +2 and +4

lead (IV) sulfide

PbS2

Palladium

Pd

BrO₄⁻¹

Perbromate

ClO₄⁻¹

Perchlorate

FO₄⁻¹

Perfluorate

IO₄⁻¹

Periodate

MnO₄⁻¹

Permanganate

O₂⁻²

Peroxide

PO₄⁻³

Phosphate

P⁻³

Phosphide

Polonium

Po

K⁺¹

Potassium

A

Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect (E) Wave nature of matter

Factors that affect the formation of a solution

Pressure Temperature Nature of Solute Nature of Solvent

Platinum

Pt

Plutonium

Pu

Combined Gas Law

P₁V₁/T₁ = P₂V₂/T₂

Universal Gas Constant

R=0.0821 (L*atm)/(mol*K)

Radium

Ra

Ra⁺²

Radium

Rubidium

Rb

Radon

Rn

Rb⁺¹

Rubidium

Sulfur

S

spontaneous if:

S > 0, H < 0, G < 0

Thiocyanate

SCN -1

thiocyanate

SCN⁻

sulfur diflouride

SF2

sulfur hexaflouride

SF6

Sulfate

SO4 -2

sulfite

SO₃²⁻

sulfate

SO₄²⁻

Antimony

Sb

Scandium

Sc

Sc⁺³

Scandium

Selenium

Se

selenium tetrabromide

SeBr4

Selenate

SeO4 -2

selenate

SeO₄²⁻

Se⁻²

Selenide

Silicon

Si

Silicate

SiO3 -2

silicate

SiO₃²⁻

SiO₃⁻²

Silicate

Si⁻⁴

Silicide

Ag⁺¹

Silver

Tin

Sn

Tin

Sn +2 and +4

tin (II) flouride

SnF2

tin(II) phosphate

Sn₃(PO₄)₂

Na⁺¹

Sodium

Strontium

Sr

strontium flouride

SrF2

Sr⁺²

Strontium

SO₄⁻²

Sulfate

S⁻²

Sulfide

SO₃⁻²

Sulfite

2nd Law of Thermodynamics

Suni=Ssurr+Ssys = 0 for nonspontaneous Suni=Ssurr+Ssys > 0 for spontaneous

Tellurium

Te

Thorium

Th

C

The Lewis dot structure of which of the following molecules shows only one unshared pair of valence electron? (A) Cl2 (B) N2 (C) NH3 (D) CCl4 (E) H2O2

D

The SbCl5 molecule has trigonal bipyramid structure. Therefore, the hybridization of Sb orbitals should be (A) sp2 (B) sp3 (C) dsp2 (D) dsp3 (E) d2sp3

Boiling-Point Elevation

The boiling point is always higher for the solution than the pure solvent

C

The cooling curve for a pure substance as it changes from a liquid to a solid is shown right. The solid and the liquid coexist at (A) point Q only (B) point R only (C) all points on the curve between Q and S (D) all points on the curve between R and T (E) no point on the curve P\ R______S \Q/ \T

A

The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom? (A) H2S (B) NH3 (C) CH4 (D) HCN (E) CO2

E

The energy change that occurs in the conversion of an ionic solid to widely separated gaseous ions (A) Activation energy (B) Free energy (C) Ionization energy (D) Kinetic energy (E) Lattice energy

C

The energy required to convert a ground-state atom in the gas phase to a gaseous positive ion (A) Activation energy (B) Free energy (C) Ionization energy (D) Kinetic energy (E) Lattice energy

Freezing-Point Depression

The freezing point is always lower for a solution of a nonvolatile solute than the pure solvent

E

The ground-state configuration for the atoms of a transition element (A) 1s2 2s2 2p5 3s2 3p5 (B) 1s2 2s2 2p6 3s2 3p6 (C) 1s2 2s2 2p6 2d10 3s2 3p6 (D) 1s2 2s2 2p6 3s2 3p6 3d5 (E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2

B

The ground-state configuration of a common ion of an alkaline earth element (A) 1s2 2s2 2p5 3s2 3p5 (B) 1s2 2s2 2p6 3s2 3p6 (C) 1s2 2s2 2p6 2d10 3s2 3p6 (D) 1s2 2s2 2p6 3s2 3p6 3d5 (E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2

B

The ground-state configuration of a negative ion of a halogen (A) 1s2 2s2 2p5 3s2 3p5 (B) 1s2 2s2 2p6 3s2 3p6 (C) 1s2 2s2 2p6 2d10 3s2 3p6 (D) 1s2 2s2 2p6 3s2 3p6 3d5 (E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2

Raoult's Law

The higher the concentration of solute particles, the less the solvent is at the interface and the lower the vapor pressure

C

The ionization energies for element X are listed in the table above. On the basis of the data, element X is most likely to be (A) Na (B) Mg (C) Al (D) Si (E) P

B

The mass of element Q found in 1.00 mole of each of four different compounds is 38.0 grams, 57.0 grams, 76.0 grams, and 114 grams, respectively. A possible atomic weight of Q is (A) 12.7 (B) 19.0 (C) 27.5 (D) 38.0 (E) 57.0

B

The melting point of MgO is higher than that of NaF. Explanations for this observation include which of the following? I. Mg2+ is more positively charged than Na+ II. O2¯ is more negatively charged than F¯ III. The O2¯ ion is smaller than the F¯ ion (A) II only (B) I and II only (C) I and III only (D) II and III only (E) I, II, and III

E

The metal calcium reacts with molecular hydrogen to form a compound. All of the following statements concerning this compound are true EXCEPT: (A) Its formula is CaH2. (B) It is ionic. (C) It is solid at room temperatur(E) (D) When added to water, it reacts to produce H2 gas. (E) When added to water, it forms an acidic solution.

B

The phase diagram above provides sufficient information for determining the (A) entropy change on vaporization (B) conditions necessary for sublimation (C) deviations from ideal gas behavior of the gas phase (D) latent heat of vaporization (E) latent heat of fusion

1st Law of Thermodynamics

The principle of the conservation of energy. Energy can be transferred and transformed, but it cannot be created or destroyed.

D

The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by weight is (A) N2O (B) NO (C) NO2 (D) N2O3 (E) N2O5

A

The structural isomers C2H5OH and CH3OCH3 would be expected to have the same values for which of the following? (Assume ideal behavior.) (A) Gaseous densities at the same temperature and pressure (B) Vapor pressures at the same temperature (C) Boiling points (D) Melting points (E) Heats of vaporization

C

The system shown above is at equilibrium at 28 °C. At this temperature, the vapor pressure of water is 28 millimeters of mercury. The partial pressure of O2(g) in the system is (A) 28 mm Hg (B) 56 mm Hg (C) 133 mm Hg (D) 161 mm Hg (E) 189 mm Hg

D

The volume of distilled water that should be added to 10.0 mL of 6.00 M HCl(aq) in order to prepare a 0.500 M HCl(aq) solution is approximately A) 50.0 mL B) 60.0 mL C) 100. mL D) 110. mL E) 120. mL

C

The weight of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution is (A) 3.10 grams (B) 12.0 grams (C) 29.4 grams (D) 294 grams (E) 300. grams

NCS⁻¹

Thiocyanate

S₂O₃⁻²

Thiosulfate

Titanium

Ti

Sn⁺²

Tin(II) or Stannous

Sn⁺⁴

Tin(IV) or Stannic

Thallium

Tl

D

Types of hybridization exhibited by the C atoms in propene, CH3CHCH2, include which of the following? I. sp II. sp2 III. sp3 (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III

Uranium

U

C

Utilized as a coating to protect Fe from corrosion (A) Pb (B) Ca (C) Zn (D) As (E) Na

A

Utilized as a shield from sources of radiation (A) Pb (B) Ca (C) Zn (D) As (E) Na

Vanadium

V

Charles's Law

V/T = k V₁/T₁ = V₂/T₂

Volume/Volume Percentage

Volume Solute/Volume Solvent

Tungsten

W

A

What is the most electronegative element? (A) O (B) La (C) Rb (D) Mg (E) N

B

When a hydrate of Na2CO3 is heated until all the water is removed, it loses 54.3 percent of its mass. The formula of the hydrate is (A) Na2CO3 . 10 H2O (B) Na2CO3 . 7 H2O (C) Na2CO3 . 5 H2O (D) Na2CO3 . 3 H2O (E) Na2CO3 . H2O

B

When a solution of sodium chloride is vaporized in a flame, the color of the flame is (A) blue (B) yellow (C) green (D) violet (E) White

E

Which element exhibits the greatest number of different oxidation states? (A) O (B) La (C) Rb (D) Mg (E) N

D

Which of the elements above has the smallest ionic radius for its most commonly found ion? (A) O (B) La (C) Rb (D) Mg (E) N

E

Which of the following acids can be oxidized to form a stronger acid? (A) H3PO4 (B) HNO3 (C) H2CO3 (D) H3BO3 (E) H2SO3

C

Which of the following actions would be likely to change the boiling point of a sample of a pure liquid in an open container? I. Placing it in a smaller container II. Increasing the number of moles of the liquid in the container III. Moving the container and liquid to a higher altitude (A) I only (B) II only (C) III only (D) II and III only (E) I, II, and III

E

Which of the following compounds is ionic and contains both sigma and pi covalent bonds? (A) Fe(OH)3 (B) HClO (C) H2S (D) NO2 (E) NaCN

A

Which of the following conclusions can be drawn from J. J. Thomson's cathode ray experiments? (A) Atoms contain electrons. (B) Practically all the mass of an atom is contained in its nucleus. (C) Atoms contain protons, neutrons, and electrons. (D) Atoms have a positively charged nucleus surrounded by an electron cloud. (E) No two electrons in one atom can have the same four quantum numbers.

A

Which of the following does NOT behave as an electrolyte when it is dissolved in water? (A) CH3OH (B) K2CO3 (C) NH4Br (D) HI (E) Sodium acetate, CH3COONa

A

Which of the following gases deviates most from ideal behavior? A) SO2 B) Ne C) CH4 D) N2 E) H2

D

Which of the following has the lowest conductivity? (A) 0.1 M CuS04 (B) 0.1 M KOH (C) 0.1 M BaCl2 (D) 0.1 M HF (E) 0.1 M HNO3

E

Which of the following is a correct interpretation of the results of Rutherford's experiments in which gold atoms were bombarded with alpha particles? (A) Atoms have equal numbers of positive and negative charges. (B) Electrons in atoms are agganged in shells. (C) Neutrons are at the center of an atom. (D) Neutrons and protrons in atoms have nearly equal mass. (E) The positive charge of an atom is concentrated in a small region.

C

Which of the following is lower for a 1.0-molar aqueous solution of any solute than it is for pure water? (A) pH (B) Vapor pressure (C) Freezing point (D) Electrical conductivity (E) Absorption of visible light

A

Which of the following is true at the triple point of a pure substance? (A) The vapor pressure of the solid phase always equal the vapor pressure of the liquid phase. (B) The temperature is always 0.01 K lower that the normal melting point. (C) The liquid and gas phases of the substance always have the same density and are therefore indistinguishable. (D) the solid phase always melts if the pressure increases at constant temperature. (E) The liquid phase always vaporizes if the pressure increases at constant temperature.

A

Which of the following molecules has a dipole moment of zero? (A) C6H6 (benzene) (B) NO (C) SO2 (D) NH3 (E) H2S

D

Which of the following pairs of liquids forms the solution that is most ideal (most closely follows Raoult's law)? A) C8H18(l) and H2O(l) B) CH3CH2CH2OH(l) and H2O(l) C) CH3CH2CH2OH(l) and C8H18(l) D) C6H14(l) and C8H18(l) E) H2SO4(l) and H2O(l)

C

Which of the following sets of quantum numbers (n, l, ml, ms) best describes the valence electron of highest energy in a ground-state gallium atom (atomic number 31) ? (A) 4, 0, 0, 1/2 (B) 4, 0, 1, 1/2 (C) 4, 1, 1, 1/2 (D) 4, 1, 2, 1/2 (E) 4, 2, 0, 1/2

E

Which of the following solids dissolves in water to form a colorless solution? (A) CrCl3 (B) FeCl3 (C) CoCl2 (D) CuCl2 (E) ZnCl2

Write the name for the formula: P₄O₁₀ Write the formula for the name: dinitrogen pentoxide

Write the formula for the name: tetraphosphorous decaoxide Write the name for the formula: N₂O₅

Write the name for the formula: AsF₃ Write the formula for the name: phosphorous pentafluoride

Write the formula for the name: arsenic trifluoride Write the name for the formula: PF₅

Write the name for the formula: BeCl₂ Write the formula for the name: arsenic trioxide

Write the formula for the name: beryllium dichloride Write the name for the formula: AsO₃

Write the name for the formula: CS₂ Write the formula for the name: boron trifluoride

Write the formula for the name: carbon disulfide Write the name for the formula: BF₃

Write the name for the formula: N₂O₄ Write the formula for the name: sulfur hexachlride

Write the formula for the name: dinitrogen tetroxide Write the name for the formula: SCl₆

Write the name for the formula: H₂O₂ Write the formula for the name: nitrogen monoxide

Write the formula for the name: hydrogen peroxide Write the name for the formula: NO

Write the name for the formula: H₂S(g) Write the formula for the name: antimony trichloride

Write the formula for the name: hydrogen sulfide Write the name for the formula: SbCl₃

Write the name for the formula: Nl₃ Write the formula for the name: carbon monoxide

Write the formula for the name: nitrogen triiodide Write the name for the formula: CO

Write the name for the formula: O₃ Write the formula for the name: nitrogen dioxide

Write the formula for the name: ozone Write the name for the formula: NO₂

Write the name for the formula: SiC Write the formula for the name: carbon tetrachloride

Write the formula for the name: silicon carbide Write the name for the formula: CCl₄

Write the name for the formula: SiO₂ Write the formula for the name: sulfur dioxide

Write the formula for the name: silicon dioxide Write the name for the formula: SO₂

Write the name for the formula: SO₃²⁻ Write the formula for the name: carbon dioxide

Write the formula for the name: sulfite ion Write the name for the formula: CO₂

Write the name for the formula: XeF₄ Write the formula for the name: sulfur trioxide

Write the formula for the name: xenon tetrafluoride Write the name for the formula: SO₃

E

X = CH3-CH2-CH2-CH2-CH3 Y = CH3-CH2-CH2-CH2-OH Z = HO-CH2-CH2-CH2-OH Based on concepts of polarity and hydrogen bonding, which of the following sequences correctly lists the compounds above in the order of their increasing solubility in water? (A) Z < Y < X (B) Y < Z < X (C) Y < X < Z (D) X < Z < Y (E) X < Y < Z

Xenon

Xe

Zn⁺²

Zinc

Zinc

Zn

Zinc

Zn +2

zinc sulfide

ZnS

Zirconium

Zr

D

__ Cr2O72¯ + __ e¯ + __ H+ ---> __ Cr3+ + __ H2O(l) When the equation for the half reaction above is balanced with the lowest whole-number coefficients, the coefficient for H2O is (A) 2 (B) 4 (C) 6 (D) 7 (E) 14

weak base

a base that reacts with water to produce hydroxide ions to only a slight extent in aqueous solution

indicator

a chemical that changes color and is used to mark the end point of a titration

oxidation state

a concept that provides a way to keep track of electrons in oxidation--reduction reactions according to certain rules

reduction

a decrease in oxidation state ( a gain of electrons)

colloid

a homogeneous mixture in which the dispersed particles do not settle out.

if Kc is large:

a large amount of products are produced, reactions lies far to the RIGHT

weak electrolyte

a material which, when dissolved in water, gives a solution that conducts only a small electric current

strong electrolyte

a material, when dissolved in water, gives a solution that conducts an electric current very efficiently

strong base

a metal hydroxide salt that completely dissociates into its ions in water

polar molecule

a molecule that has a permanent dipole moment

volumetric analysis

a process involving titration of one solution with another

oxidizing agent (electron acceptor)

a reactant that accepts electrons from another reactant

reducing agent (electron donor)

a reactant that donates electrons to another substance to reduce the oxidation state of one of its atoms

precipitation reaction

a reaction in which an insoluble substance forms and separates from the solution

oxidation-reduction (redox) reaction

a reaction in which one or more electrons are transferred

aqueous solution

a solution in which water is the dissolving medium or solvent

supersaturated solution

a solution that contains MORE dissolved solute than a saturated solution under the same conditions

unsaturated solution

a solution that contains less solute than a saturated solution under the same conditions

saturated solution

a solution that contains the maximum amount of dissolved solute

Ideal solution

a solution that obeys Raoult's law. The solute and solvent infractions are very similiar

standard solution

a solution whose concentration is accurately known

solute

a substance dissolved in liquid to form a solution

acid

a substance that marks the end point of an acid-base titration by changing color

base

a substance that produces hydroxide ions in aqueous solution, a proton acceptor

nonelectrolyte

a substance that, when dissolved in water, gives a nonconducting solution

titration

a technique in which one solution is used to analyze another

concentration (le chat)

add more products, reaction shifts left. add more reactants, reaction shifts right.

boiling point elevation

add solute, higher boiling point elevation

freezing point depression

add solute, lower freezing point depression

vapor pressure

add solute, lower vapor pressure

solubility

amount of substance needed to form a saturated solution (with a specific amt of solvent at a specific temp)

strong acid

an acid that completely dissociates to produce an H+ ion and the conjugate base

weak acid

an acid that dissociates only slightly in aqueous solution

neutralization reaction

an acid--base reaction

net ionic equation

an equation for a reaction in solution, where strong electrolytes are written as ions, showing only those components that are directly involved in the chemical change

formula equation

an equation representing a reaction in solution showing the reactants and products in undissociated form, whether they are strong or weak electrolytes

complete ionic equation

an equation that shows all substances that are strong electrolytes as ions

oxidation

an increase in oxidation state (a loss of electrons)

Cr²⁺

blue

Cu²⁺

blue

V³⁺

blue

Mn⁴⁺

brown

Cu⁺

colorless

Sc³⁺

colorless

V⁴⁺

colorless

Zn²⁺

colorless

vapor pressure _________ as imf _________

decreases, increases

viscosity _________ as temperature _________

decreases, increases

colligative properties

def properties of a solution that depend on the number of solute particles present and not on the type

does not

dilution with water does or doesn't alter the numbers of moles of solute present

H > 0

endothermic (+)

H < 0

exothermic (-)

m=moles of a solute / liters of solution

formula for molarity

moles of solute after dilution=moles of solute before dilution

formula of moles of solute after dilution

Cr³⁺

green

Fe²⁺

green

Mn⁶⁺

green

Ni²⁺

green

V³⁺

green

strength of IMFs

h-bonds > ion-dipole > dipole-dipole > LD

how to make a supersaturated solution

heat the solvent add maximum amount of solute cool down the solution

______ the concentration, _______ the chance of collisions, _______ the reaction rate

higher, greater, greater

______ temp, ______ the number of collisions, _______ the chance of collisions at the reaction site

higher, higher, greater

heats of transition _______ as imf _________

increase, increases

viscosity _________ as complexity of molecules _______

increases, increase

surface tension _________ as imf _________

increases, increases

viscosity _________ as imf _________

increases, increases

AgCl₂

insoluble

BaSO₄

insoluble

CaSO₄

insoluble

Hg₂Cl₂

insoluble

PbCl₂

insoluble

PbSO₄

insoluble

SrSO₄

insoluble

carbonates (except group 1 and ammonium)

insoluble

hydroxides (except group 1 and ammonium)

insoluble

oxides(except group 1 and ammonium)

insoluble

phosphates (except group 1 and ammonium)

insoluble

sulfides (except group 1,2 and ammonium)

insoluble

oxides (O-2)

insoluble; except group 1A and group IIA which reacts with H2O

hydroxides (OH-)

insoluble; except group 1A, Ca+2, Ba+2

carbonates (CO3-2)

insoluble; except group 1A, NH4+

phosphates (PO4-3)

insoluble; except group 1A, NH4+

sulfides (S-)

insoluble; except group 1A, group IIA, and NH4+

spectator ions

ions present in solution that do not participate directly in a reaction

nature of reactions

large, complex molecules react slower due to greater chance for collisions

immiscible

liquids that ARE NOT soluble in each other

miscible

liquids that dissolve freely in one another in any proportion

Molarity (M)

moles of solute per liter of solution M = mol / L

molarity

moles of solute per volume of solution in liters

soluble

most nitrate( NP3) salts are_______

Avogadro's Law

n/V = k n₁/V₁ = n₂/V₂

G > 0

non spontaneous

if Kc is small:

not much product is produced, reaction lies far to the LEFT

dissolve many substance

one of the most important properties of water is that it

Cr₂O₇²⁻

orange

solution equilibrium

physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates

how to mix a proper molar concentration solution

pick the size of volumetric flask to fit the solution sample size fill about half full of distilled water add the calculated amount of solute and mix until dissolved add distilled water to the fill line

Co²⁺

pink

Mn²⁺

pink

Henry's law

solubility of a gas is DIRECTLY PROPORTIONAL to the partial pressure of the gas above the liquid

Group 1 hydroxides (stong bases)

soluble

Group 1A

soluble

HBr (strong acid)

soluble

HCl (stong acid)

soluble

HClO₃(strong acid)

soluble

HClO₄(strong acid)

soluble

HI (strong acid)

soluble

HNO₃(strong acid)

soluble

H₂SO₄(strong acid)

soluble

NH4+

soluble

acetates (C₂H₃0₂)

soluble

anythiung compound with ammonium (NH₄⁺)

soluble

group 1 compouds

soluble

group 2 hydroxides below Mg

soluble

most chlorides

soluble

most sulfates

soluble

nitrates (NO₃⁻)

soluble

NO3-

soluble, except when paired with Cu+, Ag+, Pb+, Hg2+2

sulfate (SO4-)

soluble; except Pb+2, Ca+2, Sr+2, Ba+2

acetate (C2H3O2-)

soluble; except when paired with Cu+, Ag+, Pb+, Hg2+2

perchlorate (ClO4-)

soluble; except when paired with Cu+, Ag+, Pb+, Hg2+2

hydration

solution process with water as teh solvent

catalyst

speeds up a reaction by lowering the activation energy

G < 0

spontaneous

HClO3

strong acid; chloric

HBr

strong acid; hydrobromic

HCl

strong acid; hydrochloric

HI

strong acid; hydroiodic

HNO3

strong acid; nitric

HClO4

strong acid; perchloric

H2SO4

strong acid; sulfuric

Ba(OH)2

strong base

Ca(OH)2

strong base

Sr(OH)2

strong base

group IA hydroxides

strong bases (Li - Cs)

electrical conductivity

the ability to conduct an electric current

solubility

the amount of a substance that dissolves in a given volume of solvent at a given temperature

Arrhenius

the basis for the conductivity properties of a solution was first correctly identified by

solvent

the dissolving medium in a solution

osmotic pressure

the greater the difference in dissolved particles (across a membrane) the greater the osmotic pressure

boiling point elevation

the higher the number of dissolved particles the higher the boiling point

freezing point depression

the higher the number of dissolved particles the lower the freezing point

vapor pressure lowering

the higher the number of dissolved particles the lower the vapor pressure

hydration

the interaction between solute particles and water molecules

ammonia

the most common weak base is

water

the most important substances on earth is

endpoint

the point in a titration at which the indicator changes color

stoichiometric (equivalence) point

the point in a titration when enough titrant has been added to react exactly with the substance in solution being titrated

dilution

the process of adding solvent to lower the concentration of solute in a solution

precipitate

the solid formed in the precipitation reaction

half-reactions

the two parts of an oxidation--reduction reaction, one representing oxidation, the other reduction

Mn⁷⁺

violet

CH3COOH

weak acid; acetic

NH4+

weak acid; ammonium

HCN

weak acid; hydrocyanic

HF

weak acid; hydrofluoric

H2S

weak acid; hydrogen sulfide

HS-

weak base; HS- ion

NH3

weak base; ammonia

cations, anions

when ionic substances dissolve in water they break up into individual _______ and _______

Co³⁺

yellow

CrO₄²⁻

yellow

Fe³⁺

yellow

V⁵⁺

yellow


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