Unformatted text preview:

Chemistry Final Exam Study GuideChapters 1-3- Equations To Knowod=mvo˚ C=(˚ F−32˚ F)∗5 ˚ C9˚ Fo˚ F=9˚ F5˚ C∗(˚C)+32˚ FoK=(˚C +273.15)o% yield=actual yieldtheoretical yield∗100 - Scientific Notation – A systematic approach to research that begins with thegathering of information through observation and measurements. - Chemistry – The study of matter and the changes it undergoes. - Qualitative – Consisting of general observations about the system.- Quantitative – Comprising numbers obtained by various measurements of thesystem. - Hypothesis – Tentative explanation for a set of observations. - Compound – Substance composed of atoms of two or more elements chemicallyunited in fixed proportions. - Law – A concise verbal or mathematical statement of a relationship betweenphenomena that is always the same under the same conditions.- Theory – A unifying principle that explains a body of facts and/or those laws thatare based on them. - Substance – A form of matter that has a definite (constant) composition anddistinct properties. o Water, Ammonia, Gold, Oxygen. - Mixture – Combination of two or more substances in which the substances retaintheir distinct identities. o Air, Milk, Soft Drinks, Cemento Mixtures can be separated into substances through physical methods.  Homogenous Mixture – Where the composition of the mixture isthe same throughout.  Heterogeneous Mixture – Where the composition is not uniform. - Element – A substance that cannot be separated into simpler substances bychemical means. - Compound – A substance composed of atoms of two or more elementschemically united in fixed proportions. o Compounds can be separated only by chemical means into their purecomponents.- Physical Property – A property that can be measured and observed withoutchanging the composition or identity of a substance. - Chemical Property – A property where in order to observe it we must carry out achemical change. o Example: Hydrogen gas burns in oxygen gas to form water- Extensive Property – A property where the measured value depends on howmuch matter is being considered. - Mass – The quantity of matter in a given sample of a substance. - Weight – The force that gravity exerts on an object. - Volume – Length Cubed- Intensive Property – A measured value that does not depend on how muchmatter is being considered. - Density – The mass of an object divided by its volume. - Macroscopic Properties – Measurements that can be determined directly. - Microscopic Properties – Measured values that must be determined by indirectmethods on the atomic or molecular scale. - International System of Units (SI) – Metric System- Rules when Performing Arithmetic Operations in Scientific Notationo Addition or Subtraction N x 10m- Numbers need to be expressed with the same exponent(10m)- Add or subtract N1 and N2- Exponents remain the same.o Multiplication or Division N x 10m- Numbers do NOT need to be expressed with the sameexponent. - Multiply or divide N1 and N2- Add the exponents together if multiplying or subtract theexponents if dividing. - Rules for Determining Significant Figures (Sig Figs)o Any digit that is NOT zero is significant. o Zeros between nonzero digits are significant.o Zeroes to the left of the first nonzero digit are NOT significant. o If the number is greater than 1, all zeros written to the right of the decimalpoint are significant. If the number is less than 1, then only the zeros thatare at the end of the number and any zeros between nonzero digits aresignificant. o For numbers that do not contain a decimal point, the trailing zeros may ormay not be significant.  To avoid any confusion when not sure how to express an answer indecimal form, express in Scientific Notation. - How to Handle Sig Figs in Calculationso For addition and subtraction, the answer cannot have more digits to theright of the decimal point than either of the original numbers. Error is inthe last decimal place.o For multiplication and division, the number of sig figs in the final answeris determined by the original number with the LEAST number of sig figs.o Exact numbers obtained from definitions or counting contain an infinitenumber of sig figs. Chapter 2- Equations To Knowo Mass # = Number of Protons + Number of Neutronso Neutron # = Mass Number – Atomic Number- Law of Definite Proportions – Different samples of the same compound alwayscontain its constituent elements in the same proportion by mass. - Law of Multiple Proportions – If two elements can combine to form more thanone compound, the masses of one element that combine with a fixed mass of theother element are in ratios of small whole numbers. - Law of Conservation of Mass – Matter can neither be created nor destroyed. - Cation – Ion with a positive chargeo If a neutral atom loses one or more electrons it becomes a cation. - Anion – Ion with a negative chageo If a neutral atom gains one or more electrons it becomes an anion. - Ionic Compound – A compound formed from cations and anions. - Monatomic Ions – Ions that contain only one atom. o Na+, Cl-- Polyatomic Ions – Ions containing more than one atom.o OH-, CN- - Molecule – A combining of at least two atoms in a definite arrangement heldtogether by chemical forces (bonds). - Diatomic Molecule – A molecule that contains only two atoms.o H2- Polyatomic Molecule – Molecules containing more than two atoms. - Empirical Formula – Tells us which elements are present and the simplestwhole-number ration of their atoms. - Acid – A substance that yields hydrogen ions when dissolved in water. o Oxoacids – Acids that contain hydrogen, oxygen, and another element(central element). o Oxoanions – Anions of oxoacids. - Naming Oxoacids and Oxoanions- Top 10 List for Exam 1o Matter is divided into two categories: substances and mixtures. They differin the way in which they can be separated. o We use a number of prefixes to represent really large or small numbers. We can also represent these numbers using Scientific Notation. o Sig Figs are the meaningful digit in a measurement or calculated quantity. It is understood that the error is in the last digit. o Dimensional Analysis is a method to convert between units by way of conversion factors. These do not always contain an infinite number of sigfigs. It is


View Full Document

FSU CHM 1045 - Final Exam

Documents in this Course
Exam

Exam

2 pages

Notes

Notes

5 pages

Exam

Exam

4 pages

Exam

Exam

16 pages

Exam 3

Exam 3

27 pages

Notes

Notes

11 pages

Notes

Notes

2 pages

Exam 2

Exam 2

6 pages

EXAM 2

EXAM 2

7 pages

Exam

Exam

6 pages

Notes

Notes

6 pages

Notes

Notes

10 pages

EXAM 1

EXAM 1

8 pages

EXAM 1

EXAM 1

8 pages

Exam

Exam

6 pages

Chemistry

Chemistry

10 pages

Notes

Notes

10 pages

Notes

Notes

10 pages

Exam 3

Exam 3

16 pages

Chapter 1

Chapter 1

10 pages

EXAM 1

EXAM 1

8 pages

EXAM 4

EXAM 4

6 pages

EXAM 4

EXAM 4

8 pages

Chapter 2

Chapter 2

18 pages

EXAM 4

EXAM 4

8 pages

Test 3

Test 3

10 pages

EXAM 2

EXAM 2

12 pages

Exam 1

Exam 1

7 pages

Exam 1

Exam 1

7 pages

Chapter 1

Chapter 1

11 pages

Lecture 1

Lecture 1

22 pages

Exam 2

Exam 2

6 pages

Exam 1

Exam 1

48 pages

Load more
Download Final Exam
Our administrator received your request to download this document. We will send you the file to your email shortly.
Loading Unlocking...
Login

Join to view Final Exam and access 3M+ class-specific study document.

or
We will never post anything without your permission.
Don't have an account?
Sign Up

Join to view Final Exam 2 2 and access 3M+ class-specific study document.

or

By creating an account you agree to our Privacy Policy and Terms Of Use

Already a member?