Download Final Exam Review 1st Semester(All Chemistry)

Final Exam Review 1st Semester(All Chemistry)
Chapters 1-9, Nuclear Chemistry
*Items Honors
Letting Milk sour is an example of a _______________ change
The state of matter which has a indefinite shape with a definite volume is
_______________
List elements which have similar properties to Li _______________________
15.4 ml is a qualitative or quantitative observation(underline)
How many moles of H2O are present in 36 grams?
Which part of the atom is responsible for most of the mass, is positively charged
and very dense?
What is absolute zero?
Is pure water an example of a homogenous mixture?
Is salt water an example of a homgenous mixture?
Convert 30 degrees Celsius to Kelvin.
Define temperature.
**How many oxygen atoms are represented by Ba(OH)2?
**The chemical properties of an atom are related to the number of its
___________
Write the percent yield equation.
What is the law of definite proportions?
Which subatomic particles have the same mass?
56 grams of N2 gas is equal to how many moles?
**Which halide ion has the largest radius?
The total number molecules in 50 grams of water is ___________
What is the conversion factor at STP for moles to liters.
***What are the values for standard temperature Pressure?
What is the total mass of 1 mole of water?
What is the formula mass of Ca(OH)2?
What is the total number atoms in 3 moles of Li?
What is the percent composition of C in carbon dioxide?
What is the formula for lead(II) hydroxide?
Is melting exothermic or endothermic?
**Explain the law of conservation of mass and its relationship to balancing.
What type of bonds are used to form large biological molecules such as proteins?
What does (aq) mean?
What is a precipitate?
**Explain NaCl(aq) in terms of the ions
**What is the difference between soluble and insoluble?
Who discovered the electron, neutron?
What happens when electrons absorb energy?
Explain the flame test results.
**Explain how the cathode ray tube works.
How many neutron in C-14?
What is fission?
**What are transuranium elements?
**Explain how nuclear power plants operate.
**What are control rodds?
State Daltons Theory.
Define Puali exclusion principle, Heisenberg principle
What is ground and excited state?
**What is nuclear binding energy?
**What are quarks?
What is Aufbau principle?
** List the trend of the periodic table.
** do page 253 (36-39) empirical formula
Why is the atom electrically neutral?
What is the difference between C-14 and C-12?
Which element is used to set the standard for atomic mass units?
The number of atoms in 2 moles of carbon is ______________
The mass of a sample of C is 50 grams. It contains how many atoms?
According to Bohr, electrons can not reside ___________________
How did Mendeleev arrange the periodic table?
How is the periodic table arranged today?
Which groups do K and Li belong?
Name the elements that border the zig-zag line of the periodic table.
Where are the s, p, d, f blocks?
Name the groups in the f-block.
Which group has the lowest electronegativity?
Which group has the highest electronegativity?
Which group has the highest ionization energy?
Which group has the lowest ionization energy?
How many valence electrons for group 165 elements?
Where are the halogens?
The bond formed from sharing electrons _____________
The bond formed from transferring electrons _______________
The bond formed from mobile sea of electrons_______________
What is the difference between polar and nonpolar?
Is the electronegativity difference or ionization energy used to determine bond
type?
The greater the electronegativity difference the greater the ionic character(True or
False)
Which is not a molecular formula NaCl or H2O ?
In an ionic compound(crystal) cations are surrounded by ______________
Draw the lewis structure for carbon tetrachloride
Explain how hydrogen bonding occurs.
List the intermolecular forces
Write the formula for barium hydroxide
What does a chemical formula include?
Assign oxidation numbers to CH4, N2O5, OHThe mass og diamond is .30 grams and volume is .071cm3 find density
How many nitrogen atoms are there in .50 moles of NH3?
** Balance the combustion of ethane
**Pg 240 (8) average atomic mass
C+O2>>>CO2 classify the reaction and if given 24 grams of C find mass of CO2.
Write the equation hydrogen chloride and sodium hydroxide reacts to produce
sodium chloride and ___________. Balance the equation. Its is double
replacement reaction.
List and give an example of each type of reaction.
Give the mole ratio between H and O in the H2 + O2 >>> H2O
Zn + O2 >>>> ZnO How many grams of zinc oxide can be produced 70 grams of
Zinc?
In a row in the periodic table, as the atomic number increases, the atomic
radii________
**Lithium hydroxide reacts with sulfuric acid to produce lithium sulfate and
water. Given .35 kg of lithium hydroxide find mass in grams of water.
**What is a catalyst?
Why do atoms bond?
What is the octet rule?
**Give examples of polar molecules.
**Draw the orbital notation for H and chlorine and explain the bond between
HCl.
Explain the what happens to the attraction between electrons and nucleus as you
move across a period.
**Why does the electronegavity increase as you move across a period?
**Explain Millikans Oil drop experiment.
Write the symbols for alpha, beta, gamma.
List in order from smallest mass to greatest mass alpha, beta, gamma.
Which of the 3 is the most destructive.
**If the principal quantum number is 2 and angular momentum number is 1 what
are the magnetic quantum numbers? See Principal quantum number sheet
** What are symbols n,m,l see pg. 108?
From O to At the atomic radii _________
From O to At the electronegativity _________
List the states of matter in order from least KE to highest KE.
Given 5 moles of H and 3 moles of O which is the limiting reagent(reactant). H2
+ O2 >>> H2O.