Chapter 1 (Matter, Measurement, and Problem Solving)Practice Questions:1. A chemist mixes sodium with water and witnesses a violent reaction between the metal and water. This is best classified asa. an observationb. a lawc. a hypothesisd. a theory2. Which change is a physical change?a. wood burningb. iron rustingc. dynamite explodingd. gasoline evaporating3. Perform the calculation to the correct number of significant figures. (8.01-7.50)/3.002a. 0.1698867b. 0.170c. 0.17d. 0.17004. Which property of rubbing alcohol is a chemical property?a. it’s densityb. it’s flammabilityc. it’s boiling pointd. it’s melting point5. Convert 85.0 degrees F to Ka. 181.1 Kb. 358 Kc. 29.4 Kd. 302.6 KConceptsAll matter is composed of atoms and molecules.Laws, hypotheses, and theories all give rise to predictions that can be tested by experiments, carefully controlled procedures designed to produce critical new observations.A pure substance can either be an element, which cannot be chemically broken down into simpler substances, or a compound which is composed of two or more elements in fixed proportions.We can classify the properties of matter into two types: physical and chemical.In chemical and physical changes, matter often exchanges energy with its surroundings.Derived units are those formed from a combination of other units.Key EquationsK= C+273.15C= F-32/1.8D=M/VChapter 2 (Atoms and Elements)Practice Questions:1. Two samples of a compound containing elements A and B were decomposed. The first sample produced 15g of A and 35g of B. The second sample produced 25g of A and what mass of B?a. 11gb. 58gc. 21gd. 45g2. Which idea came out of Rutherford’s gold foil experiment?a. Atoms contain protons and neutronsb. Matter is composed of atomsc. Elements have isotopesd. Atoms are mostly empty space3. Determine the number of protons and neutrons in the isotope Fe-58.a. 26 protons and 58 neutronsb. 32 protons and 26 neutronsc. 26 protons and 32 neutronsd. 58 protons and 58 neutrons4. Which pair of elements do you expect to be most similar in their chemical properties?a. K and Feb. O and Sic. Ne and Nd. Br and I5. A 20.0g sample of an element contains 4.95x10^23 atoms. Identify the element.a. Crb. Oc. Mgd. FeConceptsEach element is composed of indestructible particles called atoms.All atoms of a given element have the same mass and other properties.Atoms of one element cannot change into atoms of another element. In a chemical reaction atoms change the way they are bound.Robert Millikan measured the charge of the electron, which led to the calculation of the mass of an electron.Nuclear theory states that the atom is mainly empty space, with most of its mass concentrated in a tiny region called the nucleus.Atoms are composed of three fundamental particles: the proton, the neutron, and the electron.The periodic table tabulates all known elements in order of increasing atomic number.The atomic mass of an element listed directly below its symbol in the periodic table.Key EquationsMass number= Protons+NeutronsAtomic Mass= Fraction of isotope x mass of isotope1mol= 6.0221421 x 10^23 particlesChapter 3 (Molecules, Compounds, and Chemical Equations)Exam # 1 Study Guide Lectures: 1 - 9Chapter 1 (Matter, Measurement, and Problem Solving)Practice Questions:1. A chemist mixes sodium with water and witnesses a violent reaction between the metal and water. This is best classified asa. an observationb. a lawc. a hypothesis d. a theory2. Which change is a physical change?a. wood burningb. iron rustingc. dynamite explodingd. gasoline evaporating3. Perform the calculation to the correct number of significant figures. (8.01-7.50)/3.002a. 0.1698867b. 0.170c. 0.17d. 0.17004. Which property of rubbing alcohol is a chemical property?a. it’s densityb. it’s flammabilityc. it’s boiling pointd. it’s melting pointCHEM 1211K 1st Edition5. Convert 85.0 degrees F to Ka. 181.1 Kb. 358 Kc. 29.4 Kd. 302.6 KConcepts All matter is composed of atoms and molecules. Laws, hypotheses, and theories all give rise to predictions that can be tested by experiments, carefully controlled procedures designed to produce critical new observations. A pure substance can either be an element, which cannot be chemically broken down into simpler substances, or a compound which is composed of two or more elements in fixed proportions. We can classify the properties of matter into two types: physical and chemical. In chemical and physical changes, matter often exchanges energy with its surroundings. Derived units are those formed from a combination of other units.Key Equations K= C+273.15 C= F-32/1.8 D=M/VChapter 2 (Atoms and Elements)Practice Questions:1. Two samples of a compound containing elements A and B were decomposed. The first sample produced 15g of A and 35g of B. The second sample produced 25g of A and what mass of B?a. 11gb. 58gc. 21gd. 45g2. Which idea came out of Rutherford’s gold foil experiment?a. Atoms contain protons and neutronsb. Matter is composed of atomsc. Elements have isotopesd. Atoms are mostly empty space3. Determine the number of protons and neutrons in the isotope Fe-58.a. 26 protons and 58 neutronsb. 32 protons and 26 neutronsc. 26 protons and 32 neutronsd. 58 protons and 58 neutrons4. Which pair of elements do you expect to be most similar in their chemical properties?a. K and Feb. O and Sic. Ne and Nd. Br and I5. A 20.0g sample of an element contains 4.95x10^23 atoms. Identify the element.a. Crb. Oc. Mgd. FeConcepts Each element is composed of indestructible particles called atoms. All atoms of a given element have the same mass and other properties. Atoms of one element cannot change into atoms of another element. In a chemical reaction atoms change the way they are bound. Robert Millikan measured the charge of the electron, which led to the calculationof the mass of an electron. Nuclear theory states that the atom is mainly empty space, with most of its mass concentrated in a tiny region called the nucleus. Atoms are composed of three fundamental particles: the proton, the neutron, and the electron. The periodic table tabulates all known elements in order of increasing atomic number. The atomic mass of an element listed directly below its symbol in the periodic table.Key Equations Mass number= Protons+Neutrons Atomic Mass= Fraction of isotope x mass of isotope 1mol= 6.0221421 x 10^23 particlesChapter 3 (Molecules, Compounds, and Chemical