SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
Test your basic knowledge |
CLEP Chemistry: Structure Of Matter
Start Test
Study First
Subjects
:
clep
,
science
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can
study here
.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.
This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. In chemistry - a ____ is a homogeneous mixture composed of only one phase. In such a mixture - a solute is a substance dissolved in another substance - known as a solvent. The solvent does the dissolving. The solution more or less takes on the charac
Solution
Determination of atomic masses by chemical means
Electronegativity
Evidence of Atomic Theory
2. John Dalton proposed that each chemical element is composed of atoms of a single - unique type - and though they cannot be altered or destroyed by chemical means - they can combine to form more complex structures (chemical compounds). This marked the
Atomic Spectrum
Molecular Dipolar Moments
Atomic Number
Evidence of Atomic Theory
3. ___ ___ are molecules that have the same molecular formula - but have a different arrangement of the atoms in space. That excludes any different arrangements which are simply due to the molecule rotating as a whole - or rotating about particular bond
Quantum Numbers
molecular orbital (MO) theory
Structural Isomers
Valence bond theory
4. Examples: the isotope effect is used so extensively to investigate chemical mechanisms and the use of cosmogenic isotopes and long-lived unstable isotopes in geology that it is best to consider much of isotopic chemistry as separate from nuclear chem
Evidence of Atomic Theory
Atomic Number
Valence shell electron pair repulsion (VSEPR) theory
Applications of Nuclear Chemisty
5. Electrons in a (p) orbital (either bonding or nonbonding).
resonance or mesomerism
Pi (p) electrons
Ionic Bond
Electronegativity
6. The ___ ___ of a chemical species - i.e. an atom or molecule - is the energy required to remove electrons from gaseous atoms or ions. The property is alternately still often called the ionization potential - measured in volts. In chemistry it often r
Pi Bonds
Covalent Bond
Ionization Energy
Metallic Bond
7. The mass number - also called atomic mass number or nucleon number - is the total number of protons and neutrons (together known as nucleons) in an atomic nucleus. The mass number is different for each different isotope of a chemical element.
Distinction between Periods and Groups
Atomic Number Example
Mass Number/Atomic Mass Number
Structural Isomers
8. It focuses on how the atomic orbitals of the dissociated atoms combine to give individual chemical bonds when a molecule is formed.
Atomic Theory
Atomic Orbit
Radioactive decay
valence bond (VB) theory
9. Are covalent chemical bonds where two lobes of one involved atomic orbital overlap two lobes of the other involved atomic orbital. These orbitals share a nodal plane which passes through both of the involved nuclei.
Metallic Bond
Pi Bonds
valence bond (VB) theory
Sigma (s) bonds
10. Bonds formed by the head-on overlap of sp - sp2 - or sp3 hybrid orbitals with each other or with hydrogen 1s orbitals.
valence bond (VB) theory
Ionic Bond
Sigma (s) bonds
Determination of atomic masses by chemical means
11. In chemistry - a ____ is a heterogeneous mixture containing solid particles that are sufficiently larger for sedimentation. Usually they must be larger than 1 micrometer(1mm). The internal phase (solid) is dispersed throughout the external phase (flu
Coarse Dispersion (Suspension)
Mass Spectrometry (MS) Procedure
Molecular Dipolar Moments
Radioactivity
12. __ __-__ __ (_ _ _ _)are regression models used in the chemical and biological sciences and engineering. Like other regression models - _ _ _ _models relate measurements on a set of 'predictor' variables to the behavior of the response variable.
Macromolecule
Determination of atomic masses by physical means
Quantitative structure-activity relationship models
Mass Number/Atomic Mass Number
13. In chemistry - the ____ ____ is an indicator of the degree of oxidation of an atom in a chemical compound. The formal oxidation state is the hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic. Oxid
molecular orbital (MO) theory
Oxidation State
Atomic Orbit
Atomic Weight
14. A chemical way to determine the atomic mass of an element is to combine the element with oxygen - determine the mass of the element and oxygen in the compound formed - and determine the number of atoms of oxygen combined per atom of the element.
Atomic Theory
Chemical Bond
Macromolecule
Determination of atomic masses by chemical means
15. The periodic table of the chemical elements is a list of known atoms. In the table the elements are placed in the order of their atomic numbers starting with the lowest number. The atomic number of an element is the same as the number of electrons or
The Periodic Table
Isotopes
Pi (p) bonds:
Structural Isomers
16. Formation of hybrid orbitals - which are mixtures of individual atomic orbitals. The number of atomic orbitals used to create a set of hybrid orbitals equals the number of orbitals generated by ______. Hybrid orbitals can hold up to two electrons; ha
Hybridization
Distinction between Periods and Groups
Molecular Model
Pi (p) bonds:
17. One method is the use of an auxiliary 'mass spectrometer' tube which compensates for fluctuations in both the magnetic field and the source of potential for the deflecting and accelerating plates of the main spectrometer. Ion currents are measured el
Determination of atomic masses by physical means
Pi (p) electrons
hybridisation (or hybridization)
Atomic Mass
18. A mechanism by which two atoms are held together as the result of the forces operating between them and a pair of electrons regarded as shared by them. In a ___ ___ - the electron pair occupies an orbital located mainly between the two atoms and symm
Radioactivity
Electronegativity
Sigma Bond
Determination of atomic masses by physical means
19. Describe values of conserved quantities in the dynamics of the quantum system. Perhaps the most peculiar aspect of quantum mechanics is the quantization of observable quantities - since quantum numbers are discrete sets of integers or half-integers.
Sigma (s) bonds
Radioactive decay
Determination of atomic masses by physical means
Quantum Numbers
20. A ___ ___ - in this article - is a physical model that represents molecules and their processes. The creation of mathematical models of molecular properties and behavior is ___ ___ - and their graphical depiction is molecular graphics
Molecular Dipolar Moments
Molecular Model
Coordination Complex
Pi (p) electrons
21. A ___ ___ is the attractive interaction of a hydrogen atom and an electronegative atom - such as nitrogen - oxygen or fluorine - that comes from another molecule or chemical group. The hydrogen has a polar bonding to another electronegative atom to c
Valence bond theory
Radioactive decay
Hydrogen Bond
Coordination Complex
22. __ __ are used to represent the decay of one element into another. show atomic # and mass # of particles involved. Mass numbers and atomic numbers are conserved.
Atomic Radius
Ionization Energy
Nuclear Equations
Evidence of Atomic Theory
23. Theory of bonding that states that covalent bonds form through the spatial overlap of orbitals containing valence electrons. Valence bond theory is consistent with the geometric predictions of VSEPR theory.
Atomic Spectrum
Molecular Dipolar Moments
Valence bond theory
molecular orbital (MO) theory
24. The ___ ___ of a chemical element is a measure of the size of its atoms - usually the mean or typical distance from the nucleus to the boundary of the surrounding cloud of electrons. Since the boundary is not a well-defined physical entity - there ar
Pi Bonds
Atomic Radius
Isotopes Example
Hydrogen Bond
25. Is an analytical technique that measures the mass-to-charge ratio of charged particles.[1] It is used for determining masses of particles - for determining the elemental composition of a sample or molecule - and for elucidating the chemical structure
Quantitative structure-activity relationship models
Dispersion
Mass Spectrometry (MS)
Sigma (s) bonds
26. Is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding properties. ___-ed orbitals are very useful in the explanation of the shape of molecular orbitals for molecules. It is an
Valence bond theory
Distinction between Periods and Groups
hybridisation (or hybridization)
Atomic Weight
27. The energy level of the electron is one of the things that make one state different from another. Each level - or state - has a specific energy for the electron and a specific set of probabilities for its showing up in various places.
Mass Number/Atomic Mass Number
Isotopes Example
Solution
Electron Energy Levels
28. Model for predicting molecular geometry. Based on the idea that - in a molecule - electron pairs arrange themselves as far apart as possible to minimize electron-electron repulsion. The shape of a molecule is determined by the number of electron pair
Nuclear Equations
Valence shell electron pair repulsion (VSEPR) theory
Mass Spectrometry (MS) Procedure
Hydrogen Bond
29. ___ ____ constitutes the electrostatic attractive forces between the delocalized electrons - called conduction electrons - gathered in an electron cloud - and the positively charged metal ions.
Macromolecule
Metallic Bond
Mass Spectrometry (MS) Procedure
Evidence of Atomic Theory
30. Was developed to use the methods of quantum mechanics to explain chemical bonding.molecular orbital theory has orbitals that cover the whole molecule.
Metallic Bond
molecular orbital (MO) theory
Pi (p) bonds:
Solution
31. Bohr proposed that electrons orbited the nucleus - but the electrons contained enough energy to match the electric pull of the protons. This way - the atomic stability would be preserved. He also said that electrons could occupy only certain orbits -
Atomic Number Example
Atomic Spectrum
Dispersion
Ionic Bond
32. An ___ is an atom or molecule in which the total number of electrons is not equal to the total number of protons - giving it a net positive or negative electrical charge.
Pi Bonds
Ion
Pi (p) electrons
The Periodic Table
33. A row of elements across the table is called a period. Each period has a number: from 1 to 7. Period 1 has only 2 elements in it: hydrogen and helium. Period 2 and Period 3 both have 8 elements. Other periods are longer. A column of elements down the
Distinction between Periods and Groups
Atomic Number
Covalent Bond
Macromolecule
34. Is the process by which an atomic nucleus of an unstable atom loses energy by emitting ionizing particles/radiation. A decay - or loss of energy - results when an atom with one type of nucleus - called the parent radionuclide - transforms to an atom
Quantitative structure-activity relationship models
Colloid
Atomic Mass
Radioactive decay
35. A dispersion is a system in which particles are dispersed in a continuous phase of a different composition (or state). There are three main types of dispersions: Coarse dispersion (Suspension) Colloid Solution
Coordination Complex
Macromolecule
Isotopes
Dispersion
36. A _____ is a very large molecule commonly created by polymerization of smaller subunits.
Nuclear Equations
Atomic Orbit
Macromolecule
Applications of Nuclear Chemisty
37. An ___ ___ is a type of chemical bond formed through an electrostatic attraction between two oppositely charged ions. Ionic bonds are formed between a cation - which is usually a metal - and an anion - which is usually a nonmetal
Ionic Bond
Hydrogen Bond
Nuclear Equations
Determination of atomic masses by physical means
38. A ___ ___ is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges - either between electrons and nuclei - or
Chemical Bond
Covalent Bond
Determination of atomic masses by physical means
molecular orbital (MO) theory
39. That's the number of protons in one atom of a particular element. An undisturbed atom is electrically neutral - so the number of electrons in it is the same as its atomic number. Example:
Coordination Complex
Atomic Number
Electronegativity
Quantum Numbers
40. Is a mathematical function describing the wave-like behavior of an electron in a molecule. This function can be used to calculate chemical and physical properties such as the probability of finding an electron in any specific region.
Atomic Mass
Radioactive decay
molecular orbital (MO)
Determination of atomic masses by chemical means
41. Is a way of describing delocalized electrons within certain molecules or polyatomic ions where the bonding cannot be expressed by one single Lewis formula. A molecule or ion with such delocalized electrons is represented by several contributing struc
Ion
resonance or mesomerism
Mass Spectrometry (MS) Procedure
Valence bond theory
42. A ___ ___ is an atom or ion (usually metallic) - bound to a surrounding array of molecules or anions - that are in turn known as ligands or complexing agents. Many metal-containing compounds consist of coordination complexes.
Mass Spectrometry (MS)
Mass Spectrometry (MS) Procedure
Valence bond theory
Coordination Complex
43. An explanation of the structure of matter in terms of different combinations of very small particles (atoms). is a theory of the nature of matter - which states that matter is composed of discrete units called atoms - as opposed to the obsolete notio
Ionic Bond
Atomic Theory
Distinction between Periods and Groups
Chemical Bond
44. ____ - symbol ? - is a chemical property that describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself.
Electronegativity
Mass Spectrometry (MS) Procedure
Atomic Number Example
Atomic Mass
45. ____ is the relative tendency of a bonded atom to attract electrons to itself. An atom with extremely low ____ - is said to be electropositive since its tendency is to lose rather than to gain - or attract - electrons. ______ decreases down a Group i
Electronegativity
Covalent Bond
molecular orbital (MO) theory
Colloid
46. As a general term - the mass of an individual atom; but usually we mean the average atomic mass for the naturally occurring element - expressed in atomic mass units. hydrogen and oxygen combine to form water - H2O.The weight of oxygen has to be eight
Atomic Weight
Nuclear Equations
Atomic Spectrum
Pi (p) bonds:
47. If you want to refer to a certain isotope - you write it like this: AXZ. Here X is the chemical symbol for the element - Z is the atomic number - and A is the number of neutrons and protons combined - called the mass number. For instance - ordinary h
Oxidation State
Isotopes Example
Atomic Number Example
Mass Spectrometry (MS) Procedure
48. For instance - there are two main isotopes of chlorine: chlorine-35 and chlorine-37. In any given sample of chlorine that has not been subject to mass separation there will be roughly 75% of chlorine atoms which are chlorine-35 and only 25% of chlori
Mass Number Example
Ionic Bond
Chemical Bond
Electronegativity
49. Is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom. This function can be used to calculate the probability of finding any electron of an atom in any specific region around the ato
Radioactive decay
Pi (p) bonds:
Atomic Theory
Atomic Orbit
50. Even though the total charge on a molecule is zero - the nature of chemical bonds is such that the positive and negative charges do not completely overlap in most molecules. Such molecules are said to be polar because they possess a permanent ___ ___
Molecular Dipolar Moments
Valence bond theory
Applications of Nuclear Chemisty
Mass Number/Atomic Mass Number