Sample Chem Quiz First Semester

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  • 1/39 Questions

    What did Democritus do?

    • Law of definite proportions
    • All matter is continuous
    • Discovered electron
    • All matter is made of "atoms"
    • Gold Foil Experiment discovered nucleus
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About This Quiz

The 'Sample Chem Quiz First Semester' assesses foundational knowledge in atomic structure, featuring key experiments and discoveries by scientists like Democritus, Dalton, Thomson, Rutherford, and Millikan. It covers concepts from atom composition to specific isotopes, crucial for students in chemistry.

Sample Chem Quiz First Semester - Quiz

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  • 2. 

    Who is credited with the first atomic theory?

    • Dalton

    • Rutherford

    • Democritus

    • Thomson

    • Aristotle

    Correct Answer
    A. Dalton
    Explanation
    Dalton is credited with the first atomic theory. His theory proposed that all matter is made up of tiny, indivisible particles called atoms. He also suggested that atoms of different elements have different masses and combine in simple whole number ratios to form compounds. Dalton's atomic theory laid the foundation for modern atomic theory and greatly contributed to our understanding of the structure and behavior of matter.

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  • 3. 

    Who preformed the cathode ray tube experiment and discovered the electron?

    • Dalton

    • Rutherford

    • Thomson

    • Proust

    • Newton

    Correct Answer
    A. Thomson
    Explanation
    J.J. Thomson performed the cathode ray tube experiment and discovered the electron. In this experiment, Thomson observed that cathode rays were deflected by electric and magnetic fields, suggesting the presence of negatively charged particles. He proposed that these particles were fundamental units of matter, which he called electrons. Thomson's discovery of the electron revolutionized our understanding of atomic structure and laid the foundation for the development of modern atomic theory. Dalton, Rutherford, Proust, and Newton are not associated with the discovery of the electron.

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  • 4. 

    Who preformed the gold foil experiment and discovered the nucleus?

    • Dalton

    • Thomson

    • Lavoisier

    • Newton

    • Rutherford

    Correct Answer
    A. Rutherford
    Explanation
    Rutherford performed the gold foil experiment and discovered the nucleus. In this experiment, Rutherford bombarded a thin sheet of gold foil with alpha particles. He expected the particles to pass through the foil with minimal deflection. However, some particles were deflected at large angles, and a few even bounced back. This led Rutherford to conclude that the atom has a small, dense, and positively charged nucleus at its center, surrounded by mostly empty space. This experiment revolutionized our understanding of atomic structure and laid the foundation for the modern model of the atom.

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  • 5. 

    What did Millikan's Oil Drop Experiment achieve?

    • Discovered electron

    • Discovered proton

    • Discovered atomic mass

    • Discovered mass of electron

    • Discovered neutron

    Correct Answer
    A. Discovered mass of electron
    Explanation
    Millikan's Oil Drop Experiment achieved the discovery of the mass of the electron. By observing the motion of oil droplets in an electric field, Millikan was able to determine the charge of an electron and then calculate its mass using other known values. This experiment provided crucial evidence for the existence of electrons and their fundamental properties, contributing to the development of atomic theory and our understanding of the structure of atoms.

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  • 6. 

    Given the atomic number 7, and the mass number 15, how many protons, neutrons, and electrons are there in Nitrogen - 15?

    • 2,2,2

    • 7,15,7

    • 7,8,7

    • 8,7,8

    • 15,7,15

    Correct Answer
    A. 7,8,7
    Explanation
    Nitrogen has an atomic number of 7, which represents the number of protons in the nucleus. The mass number of 15 represents the sum of protons and neutrons in the nucleus. Therefore, to determine the number of neutrons, we subtract the atomic number (7) from the mass number (15), which gives us 8 neutrons. Since the number of protons and electrons are equal in a neutral atom, there are also 7 electrons in Nitrogen-15.

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  • 7. 

    Calculate the average atomic mass:Mass (amu)              Abundance11                           97.612                           1.713                           0.7

    • 21.602 amu

    • 100.000 amu

    • 33.330 amu

    • 11.031 amu

    • 1677.559 amu

    Correct Answer
    A. 11.031 amu
    Explanation
    atomic mass % = % of isotope A/100 * Mass A + % of isotope B/100 * Mass B + % of isotope C/100 * Mass C

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  • 8. 

    What is the Electron Configuration of Carbon?

    • 1S^2 2S^2 2P^2

    • 1S 2S 3S 4S 5S 6S

    • 1S 2S 2P

    • What the heck is electron configuration? Did we even learn this?

    • None of the above

    Correct Answer
    A. 1S^2 2S^2 2P^2
    Explanation
    The correct answer is 1S^2 2S^2 2P^2. This is the correct electron configuration for carbon. The numbers and letters represent the energy levels and orbitals that the electrons occupy. The first number represents the energy level (1S is the first energy level), and the letter represents the type of orbital (S or P). The superscript number represents the number of electrons in that orbital. In the case of carbon, it has 6 electrons, so it fills the 1S orbital with 2 electrons, the 2S orbital with 2 electrons, and the 2P orbital with 2 electrons.

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  • 9. 

    What is the Electron Configuration of Cobalt?

    • 1S 2S 2P 3S 3P 4S 3D

    • 1S^2 2S^2 2P^6 3S^2 3P^6 4S^2 3D^7

    • 2 2 6 2 6 2 7

    • 1S^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10

    • None of the above

    Correct Answer
    A. 1S^2 2S^2 2P^6 3S^2 3P^6 4S^2 3D^7
    Explanation
    The electron configuration of an atom indicates how the electrons are distributed among the energy levels and orbitals. In the case of cobalt, the electron configuration is represented by the sequence of subshells filled by electrons. The given answer, 1S^2 2S^2 2P^6 3S^2 3P^6 4S^2 3D^7, represents the correct electron configuration for cobalt. It shows that cobalt has 2 electrons in the 1S orbital, 2 electrons in the 2S orbital, 6 electrons in the 2P orbital, 2 electrons in the 3S orbital, 6 electrons in the 3P orbital, 2 electrons in the 4S orbital, and 7 electrons in the 3D orbital.

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  • 10. 

    The distance from the center of an atom to th 90% probability surface of the electron is a definition of what?

    • Melting Point

    • Ionization Energy

    • Electron Affinity

    • Electronegativity

    • Atomic Radius

    Correct Answer
    A. Atomic Radius
    Explanation
    The distance from the center of an atom to the 90% probability surface of the electron is referred to as the atomic radius. It represents the size of an atom and provides information about how closely the electrons are located to the nucleus. A larger atomic radius indicates a larger atom with electrons further away from the nucleus, while a smaller atomic radius suggests a smaller atom with electrons closer to the nucleus.

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  • 11. 

    The energy required to remove an electron from an atom is a definition of what?

    • Atomic Radius

    • Electronegativity

    • Electron Affinity

    • Ionization Energy

    • Melting Point

    Correct Answer
    A. Ionization Energy
    Explanation
    The energy required to remove an electron from an atom is known as ionization energy. This energy is needed to overcome the attraction between the negatively charged electron and the positively charged nucleus of the atom. Ionization energy is an important property of an element as it determines its ability to form positive ions.

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  • 12. 

    The attraction of an atom for an electron is a definition of what?

    • Ionization Energy

    • Melting Point

    • Electron Affinity

    • Electronegativity

    • Atomic Radius

    Correct Answer
    A. Electron Affinity
    Explanation
    Electron affinity refers to the attraction that an atom has for an electron. It is defined as the energy change that occurs when an electron is added to a neutral atom in its gaseous state. A higher electron affinity indicates a stronger attraction for electrons, while a lower electron affinity suggests a weaker attraction. Therefore, electron affinity is the correct answer as it directly corresponds to the given definition.

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  • 13. 

    The relative attraction of an atom for a shared pari of electrons is a definition of what?

    • Atomic Radius

    • Electronegativity

    • Melting Point

    • Ionization Energy

    • Electron Affinity

    Correct Answer
    A. Electronegativity
    Explanation
    Electronegativity is a measure of an atom's ability to attract a shared pair of electrons towards itself in a covalent bond. It indicates the relative attraction of an atom for electrons in a chemical bond. The higher the electronegativity of an atom, the stronger its pull on the shared electrons. This property is important in determining the polarity of a bond and the distribution of electron density in a molecule.

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  • 14. 

    The temperatures at which the vapor pressures of the solid and the liquid phases of a substance are equal is the definition of what?

    • Melting Point

    • Atomic Radius

    • Ionization Energy

    • Electron Affinity

    • Electronegativity

    Correct Answer
    A. Melting Point
    Explanation
    The temperatures at which the vapor pressures of the solid and liquid phases of a substance are equal is known as the melting point. This is the temperature at which a substance changes from a solid to a liquid phase. The melting point is a characteristic physical property of a substance and can be used to identify and distinguish different substances.

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  • 15. 

    Metals have smaller ionization energies than non-metals.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Metals have smaller ionization energies than non-metals because metals have a tendency to lose electrons and form positive ions. The ionization energy is the energy required to remove an electron from an atom, and since metals have loosely held electrons in their outermost energy level, it is easier to remove these electrons. Non-metals, on the other hand, have a higher ionization energy because they have a stronger attraction for their electrons and are less likely to lose them.

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  • 16. 

    Metals have smaller electron affinities because of the shielding affect compared to non-metals which have larger electron affinities.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Metals have smaller electron affinities because of the shielding effect compared to non-metals. This means that in metals, the outermost electrons are further away from the positively charged nucleus and are shielded by inner electrons, resulting in a weaker attraction for additional electrons. Non-metals, on the other hand, have larger electron affinities because their outermost electrons are closer to the nucleus and are not shielded as effectively, leading to a stronger attraction for additional electrons. Therefore, the statement that metals have smaller electron affinities due to the shielding effect compared to non-metals is true.

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  • 17. 

    Ionic compounds form between two positive ions.

    • True

    • False

    Correct Answer
    A. False
    Explanation
    Ionic compounds actually form between a positive ion (cation) and a negative ion (anion). This is because ionic compounds are formed through the transfer of electrons from a metal (which becomes a cation) to a non-metal (which becomes an anion). The oppositely charged ions then attract each other and form an ionic bond, resulting in the formation of an ionic compound. Therefore, the correct answer is False.

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  • 18. 

    What is the name of NaCl?

    • Tin Chloride

    • Chlorine Oxide

    • Sodium Chlorine

    • Sodium Chloride

    • Sodium monochloride

    Correct Answer
    A. Sodium Chloride
    Explanation
    D is the corect ionic compound for Sodium (NA) Chloride (CL)
    E is a covalant compound

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  • 19. 

    What is the corect formula for Barium Bromide?

    • Ba Br

    • Ba2 Br

    • Ba Br2

    • IDK

    • WTF!?!

    Correct Answer
    A. Ba Br2
    Explanation
    The correct formula for Barium Bromide is BaBr2. This is because Barium has a charge of +2 and Bromide has a charge of -1. In order to balance the charges, two Bromide ions are needed for each Barium ion, resulting in the formula BaBr2.

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  • 20. 

    An ionic bond has a difference in electronegativities between to molecules of greater than 1.67.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    An ionic bond occurs when there is a large difference in electronegativities between two atoms, typically greater than 1.67. Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. In an ionic bond, one atom with a significantly higher electronegativity will attract electrons from another atom with a lower electronegativity, resulting in the formation of ions with opposite charges. This large difference in electronegativities is what allows the atoms to transfer or share electrons to achieve a stable, electrostatic attraction, making the statement true.

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  • 21. 

    What is the name of Co O2 ?

    • Cobalt Oxide

    • Cobalt (IV) Oxide

    • Cobalt (II) Oxide

    • Cobalt Oxygen

    Correct Answer
    A. Cobalt (IV) Oxide
    Explanation
    The correct answer is Cobalt (IV) Oxide. This is because the Roman numeral IV in parentheses indicates that the cobalt ion in the compound has a charge of +4. In this compound, cobalt is bonded to two oxygen atoms, so the correct name for this compound is Cobalt (IV) Oxide.

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  • 22. 

    Silver always forms an ion of 1+

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Silver always forms an ion of 1+ because it belongs to Group 11 of the periodic table, also known as the coinage metals. These metals, including silver, have a single valence electron in their outermost shell. In order to achieve a stable electron configuration, they tend to lose this electron and form a 1+ ion. Therefore, it is true that silver always forms an ion of 1+.

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  • 23. 

    Zinc always forms an ion of 2+

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Zinc always forms an ion of 2+ because it has 2 valence electrons in its outermost energy level. In order to achieve a stable electron configuration, zinc loses these 2 electrons to form a 2+ ion. This is consistent with the octet rule, which states that atoms tend to gain, lose, or share electrons in order to attain a full outer shell of electrons. Therefore, the statement "Zinc always forms an ion of 2+" is true.

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  • 24. 

    A covalant compound is only between non-metals.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    A covalent compound is formed when two or more non-metal atoms share electrons to achieve a stable electron configuration. This type of bonding occurs between non-metal elements because they have high electronegativity values and tend to gain or share electrons in order to achieve a full outer shell. In contrast, ionic compounds are formed between a metal and a non-metal, where the metal donates electrons to the non-metal. Therefore, the statement that a covalent compound is only between non-metals is true.

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  • 25. 

    What is the name for Cl2 O7 ?

    • Chlorine oxide

    • Chlorine heptoxide

    • Dichlorine oxide

    • Dichlorine heptoxide

    • Chlorine Oxygen

    Correct Answer
    A. Dichlorine heptoxide
    Explanation
    Dichlorine heptoxide is the correct answer because it accurately represents the compound Cl2O7. The prefix "di" indicates that there are two chlorine atoms, and "hept" indicates that there are seven oxygen atoms. Therefore, the name "Dichlorine heptoxide" correctly describes the composition of the compound. Chlorine oxide, chlorine oxygen, and chlorine heptoxide do not accurately represent the compound's composition.

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  • 26. 

    What is the name for the molecular formula CH4?

    • Carbon tetrahydride

    • Monocarbon tetrahydride

    • Carbon hydride

    • Methane

    • Butane

    Correct Answer
    A. Methane
    Explanation
    Methane is the correct answer because it is the name for the molecular formula CH4. Methane is a colorless and odorless gas that is the primary component of natural gas. It is the simplest hydrocarbon with one carbon atom and four hydrogen atoms, hence the molecular formula CH4.

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  • 27. 

    What does VSEPR stand for?

    • Viscosity of Slime Evolved Prudently Right

    • Valance Shell Electron Pair Repulsion

    • Valance Shell of Electron Proton Repulsion

    • This Is Stupid

    • IDK

    Correct Answer
    A. Valance Shell Electron Pair Repulsion
    Explanation
    VSEPR stands for Valence Shell Electron Pair Repulsion. This theory explains that the shape of a molecule is determined by the repulsion between electron pairs in the valence shell of the central atom. The electrons arrange themselves in a way that minimizes repulsion, resulting in specific molecular geometries.

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  • 28. 

    How many valance electrons does water have?

    • 2

    • 4

    • 6

    • 8

    • 10

    Correct Answer
    A. 8
    Explanation
    Water, with the chemical formula H2O, consists of two hydrogen atoms and one oxygen atom. Hydrogen has one valence electron, while oxygen has six valence electrons. Therefore, the total number of valence electrons in water is eight.

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  • 29. 

    What is the bond angle of a tetrahedral shape wth 4 shared pairs and 0 unshared pairs of electrons?

    • 109.5

    • 107

    • 104.5

    • 120

    • 180

    Correct Answer
    A. 109.5
    Explanation
    The bond angle of a tetrahedral shape with 4 shared pairs and 0 unshared pairs of electrons is 109.5 degrees. This is because in a tetrahedral shape, the central atom is surrounded by four other atoms or groups of atoms, creating a symmetrical arrangement. The repulsion between the electron pairs in the bonds causes them to spread out as much as possible, resulting in a bond angle of approximately 109.5 degrees.

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  • 30. 

    What is the bond angle of a trigonal pyramidol shape with 3 shared pairs and 1 unshared pair of electrons?

    • 109.5

    • 104.5

    • 107

    • 180

    Correct Answer
    A. 107
    Explanation
    In a trigonal pyramidol shape, there are 3 shared pairs of electrons and 1 unshared pair of electrons. The shared pairs repel each other, causing the bond angles to be slightly less than the ideal tetrahedral angle of 109.5 degrees. The presence of the unshared pair further compresses the bond angles. Therefore, the bond angle in this case is slightly less than 109.5 degrees, but greater than 104.5 degrees. The closest option is 107 degrees, which is the correct answer.

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  • 31. 

    What is the bond angle of a bent shape with 2 unshared pairs of electrons and 2 shared pairs of electrons?

    • 109.5

    • 107

    • 104.5

    • 180

    Correct Answer
    A. 104.5
    Explanation
    A bent shape with 2 unshared pairs of electrons and 2 shared pairs of electrons refers to a molecule with a tetrahedral electron pair geometry and a bent molecular shape. In this case, the bond angle is less than the ideal tetrahedral angle of 109.5 degrees due to the presence of the unshared pairs of electrons. The unshared pairs repel the shared pairs, causing a compression in the bond angles. Therefore, the bond angle in this case is 104.5 degrees.

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  • 32. 

    What is the bond angle of a trigonal planar shape with 3 shared pairs and 0 unshared pairs of electrons?

    • 109.5

    • 107

    • 104.5

    • 120

    • 180

    Correct Answer
    A. 120
    Explanation
    A trigonal planar shape with 3 shared pairs and 0 unshared pairs of electrons has a bond angle of 120 degrees. In a trigonal planar molecule, the three bonding pairs are arranged in a flat, triangular shape around the central atom. The repulsion between these electron pairs pushes them as far apart as possible, resulting in a bond angle of 120 degrees.

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  • 33. 

    What is the bond angle of a bent shape with 2 shared pairs of electrons and 1 unshared pair of electrons?

    • 109.5

    • 180

    • 104.5

    • 107

    Correct Answer
    A.
    Explanation
    A bent shape with 2 shared pairs of electrons and 1 unshared pair of electrons has a bond angle of 104.5 degrees. This is because the presence of the unshared pair of electrons causes greater repulsion, pushing the bonded pairs closer together and decreasing the bond angle. The bond angle of 109.5 degrees is typically associated with a tetrahedral shape, while 180 degrees is associated with a linear shape. 107 degrees is not a commonly observed bond angle for this type of arrangement.

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  • 34. 

    What is the bond angle of a linear shape with 2 shared pairs of electrons and 0 unshared pairs of electrons?

    • 109.5

    • 107

    • 104.5

    • 120

    • 180

    Correct Answer
    A. 180
    Explanation
    A linear shape with 2 shared pairs of electrons and 0 unshared pairs of electrons has a bond angle of 180 degrees. In a linear shape, the two shared pairs of electrons are located directly opposite each other, resulting in a straight line. Therefore, the bond angle is 180 degrees.

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  • 35. 

    Polar bonds can only be ina covalent bond and have an electronegativity difference of greater than or equal to 0.5.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Polar bonds occur in covalent bonds when there is an unequal sharing of electrons between atoms due to differences in electronegativity. This results in a partial positive charge on one atom and a partial negative charge on the other. The electronegativity difference between the atoms in a polar bond must be greater than or equal to 0.5. Therefore, the statement is true.

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  • 36. 

    Molecules that contain polar bonds always act as polar molecules.

    • True

    • False

    Correct Answer
    A. False
    Explanation
    False, because some molecules contain polar bonds, but the forces due to the symmetry of the molecules cancel out. For example CO2 of CF4.

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  • 37. 

    Intramolecular forces such as covalent bonds, that hold together one molecule, are the weakest of molecular forces?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    Intramolecular forces are stronger than hydrogen bonds, which are stronger than dipole-dipole forces, which are stronger than dispersion.

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  • 38. 

    Dispersion forces are the attraction between molecules due to their mass.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Dispersion forces, also known as London forces, are a type of intermolecular force that occurs between all molecules. These forces are caused by temporary fluctuations in electron distribution, resulting in temporary dipoles. These temporary dipoles induce similar dipoles in neighboring molecules, leading to an attraction between them. Dispersion forces are not dependent on the mass of the molecules but rather on their ability to polarize electron clouds. Therefore, the statement that dispersion forces are the attraction between molecules due to their mass is incorrect.

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  • 39. 

    Dipole-dipole forces are between polar molecules.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Dipole-dipole forces occur between polar molecules because these molecules have a separation of positive and negative charges, creating a dipole. The positive end of one molecule is attracted to the negative end of another molecule, resulting in an intermolecular force known as dipole-dipole force. This force is responsible for holding polar molecules together and affects their physical properties such as boiling points and solubilities. Therefore, the statement "Dipole-dipole forces are between polar molecules" is true.

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  • Nov 29, 2023
    Quiz Edited by
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  • Dec 16, 2009
    Quiz Created by
    Hayleieshorse

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