Exam 2 Chemistry

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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


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