Final Review!

What is the difference between accuracy and precision?

Who is more electronegative, Bromine or Chlorine. Why Who is more electronegative, Bromine or Chlorine? Why?? Give the electron configuration for an atom of this element.

Who has a higher ionization energy, Nitrogen or Oxygen. Why Who has a higher ionization energy, Nitrogen or Oxygen? Why? Give the electron configuraiton.

16 For an ion with isotope symbol, 32 S -2 How many protons? How many neutrons? How many electrons? What is the difference between an ion and an atom? What is the difference between an atom and an isotope?

Write the electron configuration for atoms of the following elements Phosphorus Chromium

Name that principle ________ principle - electrons enter the lowest energy first. ___________Principle - 2 electrons max per orbital - opposite spins _________’s Rule- When electrons occupy orbitals of equal energy, they don’t pair up until they have to.

How many electrons maximum can be held in the third energy level of an atom?

% Composition Calculate the Percent Composition by Mass of Sulfur in Calcium Sulfite

Empirical Formula What is the empirical formula of a compound if it is 62.1% C, 13.8% H, and 24.1% N?

Molecular Formula Find the molecular formula of ethylene glycol (antifreeze). The molar mass is 62 g/mol and the empirical formula is CH3O.

Write the formula for the following compounds Strontium nitrate Tin (II) oxide Carbon tetrafluoride Chromium (VI) carbonate

Draw structures, identify molecular geometry(shape), and polarity of the following molecules: H2S CH3Cl NH3

How many molecules are in a 14.0 g sample of CH4?

Write a balanced chemical equation for the following reaction Magnesium reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas

If 12 grams of Magnesium reacts with an excess of hydrochloric acid, how many molecules of hydrogen gas are produced?

Write a balanced chemical eqn, idenify the limiting reactant, and determine the theoretical yield of nitrogen trihydride. 23 grams of nitrogen gas react with 28 grams of hydrogen gas to produce nitrogen trihydride.

Differentiate between pure substances and mixtures Differentiate between pure substances and mixtures. Give two examples of each of the following: elements, compounds, suspensions, solutions, colloids.

List three ways to decrease reaction rate.

In the following reaction, what is the base? HBr + KOH  KBR + H2O

A high ph indicates….. An Acid A Base Salt Water

What makes a solution an Arrhenius Base??

Indicators Name an indicator and what would happen if it was in a basic solution.

According to the bronsted- lowry theory, a substance that accepts a proton in a chemical reaction is a (an)….. Base Acid Water

Identify the following substances as acidic, basic or neutral pH of 12 Sour taste Changes litmus paper blue Has high concentration of hydroxide ions (OH-1) pH of 3 Corrosive pH of 7

A solution that maintains a stable ph level would contain which of the following? pH indicator Acid Buffer Water

Is a solution with a ph of 2 a stronger or weaker acid than a solution with a ph of 4? How much stronger/weaker of an acid is it?

A gas sample at a constant pressure shrinks to one-fourth its initial volume. What must have happened to its temperature? Did it increase or decrease? By what factor did the Kelvin temperature of the gas change?

A gas occupying 2. 5 L at 25°C exerts a pressure of 0. 98 atm A gas occupying 2.5 L at 25°C exerts a pressure of 0.98 atm. What volume will it occupy if the temperature is increased to 45°C and the pressure is decreased to 93 kPa?

If a basketball stored in the garage contains 10 If a basketball stored in the garage contains 10.0 L of gas at a temperature of 20°C, what will the volume be if it is brought outside into temperatures of 0°C.

Liquids that have very high vapor pressure would likely have Strong intermolecular forces Weak intermolecular forces No intermolecular forces Very large molecules

Calculate the mass, in grams, of ice that can be melted when 8 Calculate the mass, in grams, of ice that can be melted when 8.7KJ of energy is applied to a sample of ice at 0 0C