# Final Review Chemistry HRA

 What is the molecular mass of Ni(OH)2
 a.92b. chapter 10c. mass of one moled. careful with ( )
 How many protons in Na
 a. 11b chapter 4c. protons equal atomic numberd. protons also equal electrons in a neutral atome. Atomic mass- protons= neutrons
 Write the electronic configuration for Al
 a. 1s22s22p63s23p1b. chapter 5c. pattern on periodic tabled. s hold 2 p-6 d-10 f-14e. know sectionson table
 What volume should one mole of a gas occupy at STP
 a. 22.4 litersb.chapter 10c. pv=nrt for non STP conditionsd. does not matter what type of gase; one mole of any gas occupuies the same volume under the saem conditions of temp and pressure
 What is pH of an acid
 A. LESS than 7b chapter 19c. ph measures the amount of H+d. ph= -log(H+)ph+pOH=14
 What is the charge of N in the compound NF3
 a. +3b. chapter7c in a compound total charge is zerod positive and negative must balancee. check perodic table for most likely charge. certain group-s have specific charges
 Determine the density of a liquid whose mass is 50.0 grams and the volume is 25 ml
 a. 2 grams/ mlb. chapter 3c. density = m/v then d x v = massm/d= vcheck units
 The bond angle in a water molecule is closest to?a. 180 b. 109.5 c. 105 d. 120
 a. close to 105b chapter 8c each shape has different bond anglesd.
 convet 35 grams to kg
 .035 kgchapter 2dimentional anaylsisKING HENRY
 Balance the following reactionAl + F2 —-> AlCl3
 a. 2Al + 3F2 —-> 2AlCl3b. Chapter 11c. conservation of mass
 If 2 moles Al reacts, how many moles of AlF3 form
 a. 2 molesb. Chapter 11c. coefficentw represent ratio by number nooottttttt by massd. mass- mass problems
 Which molecule is trigonal? a. H2O b, AlCl3 c. NF3 d. BrF3 1) NF3 2) H2O 3) AlCl3 4) ClF3 5) all of thes
 a.AlCl3b. chapter 8c. trigonal molecules has 120 bond angles with 3 pair of electrons.
 What is the bond angle associated with the tetrahedral shape
 a. 109.5 b. chapter 8c. every shape has different bond anglesd. tetrahedral has 4 pair of electrons in 3d
 If the hydroxide (OH) ion concentration level is .000001, then the pH is?
 a.8b. chapter 19c. log of H= pH and log (OH)= pOHd. log .000001 = 6 = pOHe. pH + pOH =14
 Determine the density of a liquid whose mass is 50.0 grams and the volume is 25 ml?
 a. 2.0 g/mlb. chapter 3c. D=m/vd. although 50.0 has 3 sig fig 25 only has 2laces of accuracy. Ans 2 places
 How many protons are present in a carbon atom?
 a. 6b. chapter 4c. protons equal atomic numberd. protons also equal electrons in a neutral atome. Atomic mass- protons= neutrons
 What is the salt created when H2SO4 and sodium hydroxide react?
 a.Na2SO4b. Chapter 19 chapter 7c. ion charges must equal zerod. Since Na is +1 and SO4 is -2 formula must be Na2SO4
 In the compound HXO3, what is the oxidation state(charge) of element X?
 a. 5b. chapter 7c in a compound total charge is zerod positive and negative must balancee. check perodic table for most likely charge. certain group-s have specific charges
 How many molecules are present in 328 grams of sodium phosphate?
 a. 1.2 x10^24 moleculesb. chapter 10c. Since the molar mass is 164, 328 is equal to 2 moles of sodium phosphate.d. 2 moles represents 6.02×10^23 *2 molecules
 What is the volume that 35.2 g of CaCO3 will occupy if it has a density of 1.60?
 a. 22.0 cm3b. Chapter 3c. there are 35.2 grams and 1.60 grams fit into one cubic centimeter, 35.2/1.60=22.0d.significant figures makes it three places of accuracy
 How many moles are in 1.81E24 atoms of K?
 a. 3b. Chapter 10 (I think)c. divide 1.81E24 by 6.02E23 to find number of moles
 What is the number of significant digits in the number 20.04080?
 a. 7b. Chapter 3c. the zero at the end is significant because it is after the decimal
 How many moles of oxygen atoms are in 1 moles of Ba(NO3)2?
 a. 6 molesb. Chapter 10c. count the number of molecules of oxygen in the formula (easy way) or do a percentage by mass equation (hard way)
 What volume would 2 moles of helium gas occupy at STP?
 a.44.8 lb. chapter 10, pg. 300c. 1 mole of gas at STp occupies a colume of 22.4d. it’s called the molar volume of the gase. STP means standard temperature and pressure
 If 2 liters of a gas at 1 atm is compressed down to 1 liter, then the new pressure should be?
 a. 2 atmb. Chapter 14: Gasesc. Boyle’s Law: PV=PVd. pressure increases when gas is compressed
 Which of the following atoms has the largest radii? a. Br B. Cl C. F D. I
 a. Ib.Chapter 6c.To find the largest radii the size generally increases going down the table and decreases going from left to right.
 How many neutrons are present in Ba-140?
 a. 84b. chapter 4, pg 111c. the neutons and protons add up to be the mass. the mass in this case is 140. the number of protons is the atomic number. so subtract 56 (the atomic number) from 140 to get 84
 How many electrons are present in U+4?
 a. 88b. Chapter 7: Ionsc. ions with a positive charges means that the element lost electrons
 How many Valence electrons does AL have?
 a.Threeb.Chapter 7c. To find the number of valence electrons in an atom of an element is to look at the group number.
 A balloon is filled to a volume of 2.0 liter is heated from 25 C to 50 C. What is the volume of the gas at a higher temperature?
 a. 2.17 litersb.chapter 14c.Charles’ Law: v1/t1=v2/t2
 what is the molar mass of NH4NO3?
 a.80gb.chapter 10c. find the mass of each element and add them together
 What is the molecular mass for baruim hydroxide?
 a. 171b. Chapter 9/10c. Ba is +2; OH is -1. d. Make formula and add weights
 How many atoms are in 2.00 mol of Na?
 a.1.20 X 10^24b.chapter 10c. in every 1 atom there is 6.02 X 10^23
 which of the following molecules is polar?a. CH4 b. CO2 c. NF3 d. BaCl2
 a. NF3b. chapter 8c. a molecule is polar when the electrons are shared unequallyd. electronegativity is the ability of a molecule to attract electrons.
 How many atoms of chloride are present in 1 mole of CaCl2?
 A.) 1.2 X 10^24B.) Chapter 10
 What is the molarity of NaOH created by dissolving 40 grams of NaOH into enough water to make 2 liters of a solution?
 a. .5Mb. Chapter 16c. Molarity is the number of moles over 1 liter solution
 the electronic configuration for Al+3 is the same as what element?
 a. Neb. chapter 5c. goal of elements are to be completly stable like Noble Gases.
 38.) What is the molarity of a solution with 41.6 CaCl2 in 750.0 cm^3 of water?
 A.) .5MB.) Chapter 16
 How much would 2 moles of carbon dioxide weigh?
 a. 88gb Chapter 10c. atomic mass x # of moles is the weight in grams
 What is the concentration of hydronium ion if the pH is 3.6 ?
 a. 2.5 x 10^-4 Mb. Chapter 19c. [H+]= 10^-pHd. don’t forget the negative sign
 What is the pHO for a solution containing 2.5 x 10^-4 M hydroxide ions ?
 a. 3.6b. Chapter 19c. pHO= -log[OH-]d. dont forget the negative sign
 Which atom is most similar in its properties to Barium? a)Hydrogen b)Lithium c)Cesium d)Strontium
 A)StrontiumB)chapter 6C)elements of the same group are similar
 10*C is equal to what in Kelvin.
 a. 283*Kb. chapter 8c. K=C+273
 What is the shape of a molecule of NBr5?
 a. trigonal bipyramidb. chapter 8c. N is +5d. Br is -1e. five atoms of Br off of N
 Consider a sealed cylinder with a moveable piston inside. As the piston moves down, the pressure inside the cylinder should a)increase b)decrease c)stays the same
 A) increasesB) chapter 14C) as the piston moves down, the volume decreases but the amount of “stuff” there stays the same
 Which of the following contains the greatest number of atoms ? 1.) 2.5 moles of Sodium 2.) 1.5 grams of Nickel 3.) 22.4 liters of Neon at STP 4.) 3.0 grams of Sodium
 a. 2.5 moles of Sodiumb. chapter 10c. find out the number of moles of each d. the greater number of moles the greater the number of atoms
 How many moles of gas would occupy a sealed 2.0 liter flask at a pressure of 2.0 atmospheres and a temperature of 373K
 a. .131b. PV=NRTc.R= .0821 because pressure of atm
 the outermost electron configuration of hafnium is ?
 a. 5d2b. chapter 5 c. memorize what group it is ind. memorize the order they go in on the peridoic table
 Which of the following ions is the largest? a.Na+ b. Mg+2 c. Fe+2 d. Br-
 a.Br-b. Chapter 6 c. There is an extra electron added to bromine. d. look at location on the periodic table and atomic weight.
 How would we name the compound Fe2O3?
 a. Iron(III)Oxideb. Chapter 9c. Don’t forget roman numerals
 How many electrons can the 4th level hold?
 a. 32b. chapter 5c. s=2 p=6 d=10 f=14 2+6+10+14=32
 How would we name the compound Fe2O3?
 a. Iron(III)Oxideb. Chapter 9c. Don’t forget roman numerals
 How would we name the compound Fe2O3?
 a. Iron(III)Oxideb. Chapter 9c. Don’t forget roman numerals
 The temperature at STP should be:
 a. 273 Kb. chapter 10c. STP=0 degrees Cd. Celcius + 273 = degrees Kelvin
 According to Bronsted and Lowry, acids are proton:
 a. donorsb. chapter 19
 Which molecule is not polar?a. HBr b. H2O c. NH3 d. CCl4
 a. CCl4b. Chapter 5 c. non polar molecules do not have any unbonded pairs of electrons.
 Which sublevel contains a maximum of 5 pairs of electrons?
 a. db. Chapter 5c. pairs=2
 The bonding in ethane is? (C2H6)
 a. Nonpolar Covalentb. Chapter 8c. Electronegativity
 What is the electron configuration for gallium?
 a. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p1b. Chapter 5c. Look at columns
 An atom with a charge is called an?
 a. Ionb. Chapter 6 c. Don’t be stupid JPd. + ions have fewer electronse. – ions have more electrons
 Covalent bonds are characterized by:
 a. shared electronsb.chapter 8c.covalent relates to two electrons d. in order to be covalent, they need to be shared.
 Oxygen has a volume of 1.429 dm3 at STP. Which of the following will result in the greatest change in volume?
 a. doubling the temperature and halving the pressureb. chapter 13c. pv=nrt (do it multiple times)
 What is the new volume of a gas that occupies 45.0 cm^3 at 49 C when it is cooled to -29 C if the pressure remains constant?
 a. 34.1 cm^3b. Chapter 13c. V/t=v/tD. convert to K
 A molecure having 3 shared pairs of electrons and one unshared pair of electrons would have this shape:
 a. irregular tetrahedralb. chapter 8c.at least trigonal because there are 3 pairs of covalent bondd. the unshared electrons add another side making it tetrahedrale. its irregular becuase the fourth side is unshared.
 Which of the following gases has the greatest rate of diffusion (speed) if all are at the same temperature and pressure?
 a. hydrogenb. chapter 13c. small is the fast
 Which of the following bonds would be ionic?a. CH4 b. NO2 c. XeF6 d. MgCl2
 a. d, MgCl2b. Chapter 7c. Larger the electronegativity, the more ionicd. opposite sides of the periodic table
 How many electrons are in a double bond?
 a. fourb. Chapter 8c.a double bond is two PAIRS of electrons.d. remember the octet rule
 What is the maximum number of electrons that may occupy one orbital?
 a. twob. Chapter 5c. look at Table 5.1 on pg. 131 and Table 5.3 on pg. 134 both in the textbook
 Which atom has a half full sub-level?1)Ni 2)p 3)La 4)U 5)Ne
 a. Pb. Chapter 5.2c. the p level has 6 sublevels and Phosphorus has three sub levels, so it’s half full.
 If an atom loses electrons, its charge is?
 a. positiveb. chapter 4c. positive atoms have more protons then electrons, so they have to give away electrons to become positive.
 How many atoms are present in 28 grams of silicon?
 a. 6.02*10E23b. chapter 10c. make your triangle with moles, volume and number of atoms. divide the grams by the weight of silicon, then multiply it times 6.02*10^23
 Which compound is the most polar? a. CO b. CaO c. KF d. CaI e. LiH
 a. KFb. Chapter 11c. Remember Fluorine has a very high elctronegativity!
 What is the concentration of Hydrodium (H+) ions in a neutral solution at 25 C?
 a. 1X10E-7b. chapter 16c. neutral solutions have equal Hydronium and Hydroxide concentrations.
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