Exam 2 Chemistry
a. increases b. decreases c. increases
A gas with a volume of 4.0 L is in a closed container. Indicate the changes in its pressure when the volume undergoes the following changes at the same temperature and amount of gas: a. The volume is compressed to 2.0 L b. The volume expands to 12 L c. The volume is compressed to 0.40 L
b. 29.4 lb/in2 c. 1520 mmHg d. 203 kPa
A tank contains oxygen (O2) at a pressure of 2.00 atm. what is the pressure in the tank in terms of the following units? b. lb/in2 c. mmHg d. kPa
In a gas mixture, the pressure that each gas exerts as part of the total pressure is called the partial pressure of that gas. Because the air sample is a mixture of gases, the total pressure is the sum of the partial pressures of each gas in the sample>
A typical air sample in the lungs contains oxygen at 100 mmHg, nitrogen at 573 mmHg, carbon dioxide at 40 mmHg, and water vapor at 47 mmHg. Why are these pressures called partial pressures?
alkaline earth metals
Found in Group 2A including the elements beryllium, magnesium, calcium, strontium, barium, and radium
noble gases
Found in Group 8A; include helium, neon, argon, krypton, xenon, radon
Iron (III) oxide Potassium chloride Copper (II) oxide Silver sulfide
Give the name of the compounds with the following formulas: Fe2O3 KCl CuO Ag2S
He Na Al
Give the symbol of the element described by each of the following the noble gas in Period 1 the alkali metal in Period 3 group 3A period 3
Metalloids
Besides aluminum the elements along the heavy line; semiconductors, can be modified to function as conductors or insulators, share some characteristics of both metals and nonmetals
CO2 SiO2 N2O5 SO2 PCl3
Carbon dioxide Silicon dioxide Dinitrogen pentoxide Sulfurdioxide Phosphorus trichloride
CoBr2- ionic SiCl4 - covalent Fe3P2- ionic H2O- covalent AlI3- ionic
Classify each compound as covalent or ionic and then provide the formula: Cobalt (II) bromide Silicon tetrachloride iron (II) phosphide dihydrogen monoxide aluminum idodide
Period
Each horizontal row in the periodic table is a ______
Group
Each vertical column on the periodic table is called______ which is composed of elements that have similar properties
gaining electrons negatively charged
nonmetals form ions by ________ electrons nonmetal ions are _______ charged
Nonmetals
not especially shiny, ductile or malleable, poor conductors of heat and electricity, low melting points, low densities
group number
Valence electrons for main group elements can be determined by?
H2, N2, O2, F2, Cl2, Br2, I2
What are the 7 diatomic elements?
chemical bonds
What do the unpaired valence electrons form?
Helium the two dots go together on the right side
What element is the exception to the rules of the lewis symbol method? Where do the dots go?
a. atomic b. both c. mass d. atomic
When would you use the atomic number , mass number, or both to determine each of the following? a. number of protons in an atom b. number of neutrons in the atom c. number of particles in the nucleus d. number of electrons in a neutral atom
a, d, e
Which of the following statements describe the pressure of a gas: a.The force of the gas particles on the walls of the container b. the number of gas particles in a container c. 4.5 L of helium gas d. 750 torr e. 28.8 lb/in2
Dalton's Atomic Theory
1. All matter is made up of tiny particles called atoms 2. All atoms of a given element are the same and different from atoms of other elements 3. Atoms of two or more different elements combine to form compounds. A particular compound is always made up of the same kinds of atoms and always has the same number of each kind of atom 4. A chemical reaction involves the rearrangement, separation, or combination of atoms. Atoms are neither created nor destroyed during a chemical reaction
a. 328 mmHg b. 2620 mmHg
A 10.0 L balloon contains helium gas at a pressure of 655 mmHg. What is the final pressure, in mmHg, when the helium is placed in tanks that have the following volumes, if there is no change in temperature and amount of gas? a. 20.0 L b. 2.50 L
Metalloids
B, Si, Ge, As, Sb, Te, Po, At, Ts along the heavy line disregarding aluminum
4Al + 3O2= 2Al2O3 H2SO4 + 2NH4OH = 2H2O + (NH4)2SO4
Balance these chemical equations: Aluminum + Oxygen = Aluminum oxide H2SO4 + NH4OH = H2O + (NH4)2SO4
alkali metals
Group 1A consisting of lithium, sodium, potassium, rubidium, cesium and francium are a family of elements known as __________ (disregard hydrogen)
Representative elements
Group numbers 1A through 8A are called
1, 2, 8
How many valence electrons are in each? Group 1A Group 2A Group 8A
a. electron b. proton c. electron d. neutron
Identify each of the following as describing either a proton, a neutron, or an electron a. has the smallest mass b. has a 1+ charge c. is found outside the nucleus d. is electrically neutral
metal metal nonmetal nonmetal metalloid metal
Identify each of the following elements as a metal, a nonmetal, or a metalloid: Calcium a shiny element an element that is a gas at room temperature located in Group 8A Boron silver
a. temperature b. volume c. amount d. pressure
Identify the property of a gas that is measured in each of the following: 350 K 125 mL 2.00 g of O2 755 mmHg
Transition elements
In the center of the periodic table is a block of elements known as the
1. +1 2. +2 3. +3 4. -1 5. -2 6. -3
Ionic charges can be determined by group number: 1. Group 1= 2. Group 2= 3. Al in group 3A= 4. Group 7A= 5. Group 6A= 6. Group 5A nonmetals=
a. true b. true c. true d. false; a proton is attracted to an electron
Is each of the following statements true or false? a. a proton and an electron have opposite charges b. the nucleus contains most of the mass of an atom c. electrons repel each other d. a proton is attracted to a neutron
a. aluminum sulfate (ionic) b. Calcium carbonate c. Dinitrogen monoxide d. Magnesium hydroxide
Name each of the following ionic or molecular compounds: a. Al2(SO4)3 b. CaCO3 c. N2O d. Mg(OH)2
a. sulfate b. carbonate c. hydrogen sulfite d. nitrate
Name the following polyatomic ions: a. SO4 (2-) b. CO3 (2-) c. HSO 3 (-) d. NO3 (-)
iodine trichloride sulfur hexafluoride silicon dioxide tetraphosphorous heptasulfide
Prove the formulas for the following covalent compounds: ICl3 SF6 SiO2 P4S7
Barium nitrate Aluminum chloride Potassium oxide Calcium hydroxide
Provide the names for the following ionic compounds: Ba(NO3)2 AlCl3 K2O Ca(OH)2
b. 3 electrons gained c. 1 electron gained e. 1 electron gained
State the number of electrons lost or gained when the following elements form ions: b. P c. Group 7A (17) e. Br
Rubidium (Rb), Strontium (Sr), Palladium (Pd), Silver (Ag), Tin (Sn), Iodine (I), Xenon (Xe)
The fifth period contains 18 elements but only have to know 7 of them: (Disregard y, zr, nb, mo, tc, ru, rh, cd, in, sb, te)
Hydrogen (H) and Helium (He)
The first period contains two elements:
potassium (K), calcium (Ca), scandium (Sc), titanium (Ti), vanadium (V), chromium (Cr), manganese (Mn), iron (Fe), cobalt (Co), nickel (Ni), copper (Cu), zinc (Zn), arsenic (As), selenium (Se), bromine (Br), krypton (Kr)
The fourth period contains 18 elements but only have to know 16 of them: (Disregard Ga and Ge)
lithium (Li), beryllium (Be), boron (B), carbon (C), nitrogen (N), oxygen (O), fluorine (F), and neon (Ne)
The second period contains eight elements:
sodium (Na), magnesium (Mg), aluminum (Al) silicon (Si) phosphorus (P) sulfur (S) chlorine (Cl) and argon (Ar)
The third period also contains eight elements:
a. At higher temperature, gas particles have greater kinetic energy, which makes them move faster b. Because there are great distances between the particles of a gas, they can be pushed closer together and still remain a gas c. Gas particles are very far apart, which means that the mass of a gas in a certain volume is very small, resulting in a low density.
Use the kinetic molecular theory of gases to explain each of the following: a. Gases move faster at higher temperatures b. Gases can be compressed much more easily than liquids or solids. c. Gases have low densities
As a diver ascends to the surface, external pressure decreases. If the air in the lungs were not exhales, its volume would expand and severely damage the lungs. The pressure in the lungs must adjust to changes in the external pressure.
Why do scuba divers need to exhale air when they ascend to the surface of the water?
1. 2Cu + O2= 2CuO 2. C3H8 + 5O2= 3CO2 + 4H2O
Write a balanced chemical equation for the following: copper reacts with oxygen to produce copper (II) oxide (CuO) Propane (C3H8) reacts with oxygen to produce carbon dioxide and water
a. Ba (OH)2 c. Fe (NO2)2 e. Fe2(CO3)3
Write the correct formula for the following ionic compounds: a. barium hydroxide c. iron (II) nitrite e. iron (III) carbonate
a. Na2O b. AlBr3 c. Ba3N2 d. MgF2 e. Al2S3
Write the correct ionic formula for the compound formed between each of the following pairs of ions: a. Na+ and O2- b. Al 3+ and Br- c. Ba 2+ and N3- d. Mg 2+ and F- e. Al 3+ and S 2-
a. K3P b. CuCl2 c. FeBr3 d. MgO
Write the formula for each of the following ions: a. potassium phosphide b. copper (II) chloride c. iron (III) bromide d. magnesium oxide
a. OF2 b. BCl3 c. N2O3 d. SF6
Write the formula for each of the following molecular compounds: a. oxygen difluoride b. boron trichloride c. dinitrogen trioxide d. sulfur hexafluoride
a. HCO3- b. NH4+ c. PO3 (3-) <---(superscript) d. ClO3 -
Write the formula including the charge for each of the following polyatomic ions: a. hydrogen carbonate (bicarbonate) b. ammonium c. phosphite d. chlorate
aluminum fluoride sodium oxide potassium iodide
Write the name for each of the following ionic compounds: a. AlF3 c. Na2O e. KI
a. Iron (II) c. zinc e. chromium (III)
Write the name for each of the following ions (include roman numeral when necessary): a. Fe 2+ c. Zn 2+ e. Cr 3+
a. Cl- b. Cs+ c. N 3- d. Ra 2+
Write the symbol for the ion of each of the following: a. chlorine b. cesium c. nitrogen d. radium
b. F- c. Mg2+
Write the symbols for the ions with the following number of protons and electrons: b. 9 protons, 10 electrons c. 12 protons, 10 electrons
Non polar covalent bond
a bond between two of the same nonmetal or a C-H bond *pair of electrons shared equally by both atoms
Ionization energy
a quantity of energy that is required to remove one of the outermost electrons
metallic character
an element that loses valence electrons easily more common with metals on the left side of the periodic table and decreases going from left to right across a period
Subatomic particles
atoms composed of smaller bits of matter called
Isotopes
atoms of the same element that have the same atomic number but different numbers of neutrons
Metals
copper (Cu), gold (Au), and silver (Ag) are examples of what kinds of elements?
neutron
electrically neutral, same mass as a proton
absorb
electrons can move to higher energy levels when they _______(absorb/emit) energy
Valence electrons
electrons in the outermost energy level
Group 1A alkali metals
elements within this group are soft, shiny metals that are good conductors of heat and electricity and have relatively low melting points and react vigorously with water
Atomic number
equal to the number of protons in every atom of that element, appears above the symbol of each element on the periodic table
Covalent bonds
form when atoms of nonmetals share valence electrons
halogens
found on the right side of the periodic table in Group 7A; include fluorine, chlorine, bromine, iodine, astatine
metals on the left nonmetals on the right
heavy zigzag line separates the elements into ______ on the left and _____ on the right
Group 7A Halogens
highly reactive, especially fluorine and chlorine, and form compounds with most of the elements
Nonmetals
hydrogen, carbon, nitrogen, oxygen, chlorine, and sulfur are examples of what kinds of elements?
ionic bonds
in ionic compounds between metal and nonmetal; stronger than covalent bonds
protons
in nucleus, positive charge, much larger than electron
atomic symbol
indicates the mass number in the upper left corner and the atomic number in the lower left corner to distinguish between the different isotopes of an element
cations anions
metal ions are are positively charged ions called nonmetal atoms are negatively charged ions called
losing electrons positive charges
metals form ions by______ metal ions have ____ charges
Ionic bonds
occur when the valence electrons of atoms of a metal are transferred to atoms of nonmetals
Chemical symbols
one- or two-letter abbreviations for the names of the elements
Polar covalent bond
pair of electrons is not shared equally between 2 different nonmetal atoms, partial charges, but not really ionic *The atom with more nonbonding electron pairs is the partially negative atom or *the atom closer to the fluorine in the periodic table is the partially negative atom
nucleus
positively charged region at the center of the atom
Group 8A Noble Gases
quite unreactive and are seldom found in combination with other elements
Metals
shiny solids, can be shaped into wires (ductile) or hammered into a flat sheet (malleable), good conductors of heat and electricity, melt at high temperatures, solid at room temperature, except for mercury
electron
small mass, outside of the atom, charge: -1
a. 1 b. 2 d. 1
state the number of electrons that must be lost by atoms of each of the following to achieve a stable electron arrangement: a. Li b. Ca d. Cs
Proton: p+, 1+, 1.007 amu, nucleus Neutron: n, 0, 1.008 amu, nucleus Electron: e-, 1-, 0.00055 amu, outside nucleus
subatomic particles in the atom symbol, charge, mass, location
Electron, proton, neutron
subatomic particles; two discovered because they have electrical charges
Group 1A: 1 valence electron Group 2A: 2 valence electrons Group 7A (halogens): 7 valence electrons
the group number gives the number of valence electrons for each group of representative elements How many valence electrons are in each: Groups 1A, 2A and 7A
decreases
the ionization energy ________ going down a group
Atom
the smallest particle of an element that retains the characteristics of that element
Ions
these have electrical charges, they form when atoms lose or gain electrons to form a stable electron arrangement
Group 2A alkaline earth metals
these metals are shiny metals, but not as reactive as the others
Lewis symbol They get paired with the other ones
this is a convenient way to represent the valence electrons as dots, which are placed on the sides, top or bottom of the symbol for the element if it contains 5-8 valence electrons what happens to the electrons?
atomic mass
this is the average of the masses of the naturally occurring isotopes of that element On the periodic table, this is the number including decimal places that is given below the symbol of each element
Mass number
total number of protons and neutrons in the nucleus
b. Group 7A, 7 electrons d. Group 5A, 5 electrons f. Group 3A, 3 electrons
what is the group number and number of valence electrons for each of the following elements? b. iodine d. phosphorus f. boron
cation
when an electron is removed from a neutral atom, a positive particle with a 1+ charge is formed
a. 2,8,6 b. 2,8,1 c. 2,5 d. 2,8,8,1
write the electron arrangement for the following elements: a. sulfur b. sodium c. nitrogen d. potassium
a. tin (II) chloride b. iron (II) oxide c. copper (I) sulfide d. copper (II) sulfide e. cadmium bromide f. mercury (II) chloride
write the name for each of the following ionic compounds: a. SnCl2 b. FeO c. Cu2S d. CuS e. CdBr2 f. HgCl2
K+ and S2- K2S Na + and N 3- Na3N Al 3+ and I-, AlI3 Ga 3+ and O 2- Ga2O3
write the symbols for the ions, and the correct formula for the ionic compound formed by each of the following: a. potassium and sulfur b. sodium and nitrogen c. aluminum and iodine d. gallium and oxygen
Group number
written at the top of each vertical column in the periodic table