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Test your basic knowledge |
CLEP Chemistry: Structure Of Matter
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Subjects
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clep
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science
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chemistry
Instructions:
Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can
study here
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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. ___ ____ constitutes the electrostatic attractive forces between the delocalized electrons - called conduction electrons - gathered in an electron cloud - and the positively charged metal ions.
Metallic Bond
Atomic Number
Atomic Number Example
Mass Number/Atomic Mass Number
2. 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
Atomic Theory
Mass Spectrometry (MS)
Isotopes Example
Electronegativity
3. 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
Sigma Bond
molecular orbital (MO)
Mass Spectrometry (MS) Procedure
Coarse Dispersion (Suspension)
4. 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
Atomic Spectrum
Evidence of Atomic Theory
Electron Energy Levels
Hydrogen Bond
5. 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.
Distinction between Periods and Groups
Solution
Dispersion
Ion
6. 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
Evidence of Atomic Theory
Structural Isomers
Macromolecule
Molecular Model
7. A _____ is a very large molecule commonly created by polymerization of smaller subunits.
Solution
Macromolecule
Isotopes Example
Radioactive decay
8. 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
Valence shell electron pair repulsion (VSEPR) theory
Oxidation State
Pi Bonds
Ion
9. ___ ___ 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
Sigma Bond
Structural Isomers
Electronegativity
Pi (p) bonds:
10. 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
Chemical Bond
The Periodic Table
Ionic Bond
valence bond (VB) theory
11. (1) A sample is loaded onto the MS instrument and undergoes vaporization (2) The components of the sample are ionized by one of a variety of methods (e.g. - by impacting them with an electron beam) - which results in the formation of charged particle
Electronegativity
Mass Spectrometry (MS) Procedure
Covalent Bond
Electron Energy Levels
12. __ __ 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.
Mass Number/Atomic Mass Number
Nuclear Equations
Quantitative structure-activity relationship models
Valence shell electron pair repulsion (VSEPR) theory
13. 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
Quantum Numbers
Hybridization
Determination of atomic masses by physical means
Distinction between Periods and Groups
14. A ____ is a substance microscopically dispersed evenly throughout another substance.A colloidal system consists of two separate phases: a dispersed phase (or internal phase) and a continuous phase (or dispersion medium) in which the colloid is disper
Colloid
Atomic Orbit
Mass Spectrometry (MS)
Distinction between Periods and Groups
15. 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.
Quantum Numbers
Electron Energy Levels
molecular orbital (MO)
Sigma (s) bonds
16. 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.
Coordination Complex
resonance or mesomerism
Molecular Model
hybridisation (or hybridization)
17. 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
Quantitative structure-activity relationship models
Sigma Bond
Isotopes
18. 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
Isotopes Example
Applications of Nuclear Chemisty
Atomic Radius
Valence shell electron pair repulsion (VSEPR) theory
19. ____ - symbol ? - is a chemical property that describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself.
molecular orbital (MO) theory
Electronegativity
Mass Spectrometry (MS) Procedure
Macromolecule
20. Was developed to use the methods of quantum mechanics to explain chemical bonding.molecular orbital theory has orbitals that cover the whole molecule.
Mass Number/Atomic Mass Number
Radioactivity
Structural Isomers
molecular orbital (MO) theory
21. The mass of an atom of a chemical element expressed in atomic mass units (amu). It is approximately equivalent to the number of protons and neutrons in the atom (the mass number) or to the average number allowing for the relative abundances of differ
Determination of atomic masses by chemical means
Pi Bonds
Atomic Theory
Atomic Mass
22. The atomic number of hydrogen is 1; the atomic number of carbon is 6. The atomic number is also known as the proton number. It may be represented by the capital letter Z.
Isotopes Example
Nuclear Equations
Atomic Number Example
Macromolecule
23. 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
Quantitative structure-activity relationship models
Atomic Spectrum
Ionization Energy
Isotopes
24. 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.
Structural Isomers
Electron Energy Levels
Mass Number Example
Molecular Dipolar Moments
25. 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
Sigma (s) bonds
Valence shell electron pair repulsion (VSEPR) theory
Atomic Weight
Distinction between Periods and Groups
26. 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
Pi Bonds
Atomic Spectrum
Determination of atomic masses by physical means
Ion
27. 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
resonance or mesomerism
Electronegativity
Atomic Spectrum
molecular orbital (MO) theory
28. 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
Sigma Bond
hybridisation (or hybridization)
Distinction between Periods and Groups
Evidence of Atomic Theory
29. 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
Molecular Model
Dispersion
hybridisation (or hybridization)
Electron Energy Levels
30. 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 -
Ionic Bond
Atomic Number Example
Nuclear Equations
Atomic Spectrum
31. 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.
Determination of atomic masses by chemical means
Hydrogen Bond
Quantum Numbers
Quantitative structure-activity relationship models
32. ____ 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
Radioactive decay
Electronegativity
Coarse Dispersion (Suspension)
The Periodic Table
33. 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
Ionic Bond
Valence bond theory
Electronegativity
Radioactive decay
34. 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
Mass Number Example
Structural Isomers
Determination of atomic masses by chemical means
Atomic Theory
35. 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.
Hybridization
Pi Bonds
Mass Number/Atomic Mass Number
Radioactive decay
36. 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
Isotopes
Atomic Orbit
Ion
Chemical Bond
37. 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.
Ionization Energy
Pi Bonds
Hybridization
Coarse Dispersion (Suspension)
38. 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
Coarse Dispersion (Suspension)
Dispersion
Determination of atomic masses by physical means
39. 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.
Evidence of Atomic Theory
Oxidation State
Valence bond theory
Quantitative structure-activity relationship models
40. It focuses on how the atomic orbitals of the dissociated atoms combine to give individual chemical bonds when a molecule is formed.
Colloid
valence bond (VB) theory
Ionic Bond
Ionization Energy
41. 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:
Atomic Orbit
Atomic Number
Dispersion
Atomic Theory
42. 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
Atomic Radius
Metallic Bond
Atomic Spectrum
molecular orbital (MO)
43. Atoms of the same element can have different numbers of neutrons; the different possible versions of each element are called isotopes. For example - the most common isotope of hydrogen has no neutrons at all; there's also a hydrogen isotope called de
hybridisation (or hybridization)
Atomic Spectrum
Isotopes
Mass Spectrometry (MS)
44. 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
Pi (p) electrons
Atomic Spectrum
Ion
Atomic Weight
45. Electrons in a (p) orbital (either bonding or nonbonding).
Sigma (s) bonds
Pi (p) electrons
Sigma Bond
Electronegativity
46. 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
Oxidation State
Metallic Bond
hybridisation (or hybridization)
Atomic Spectrum
47. 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
Sigma Bond
Radioactive decay
Atomic Orbit
Coarse Dispersion (Suspension)
48. 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
Sigma Bond
Oxidation State
Molecular Model
Atomic Weight
49. 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.
Valence shell electron pair repulsion (VSEPR) theory
Isotopes
Nuclear Equations
molecular orbital (MO)
50. A ___ ___ is a form of chemical bonding that is characterized by the sharing of pairs of electrons between atoms. The stable balance of attractive and repulsive forces between atoms when they share electrons is known as covalent bonding.
Oxidation State
Sigma (s) bonds
Covalent Bond
Determination of atomic masses by physical means