Term
| Which two particles make up most of the mass of a hydrogen-2 atom |
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Definition
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Term
| In the wave-mechanical model of the atom,orbitals are regions of the most probable locations of |
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Definition
|
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Term
| Which phrase describes an atom? |
|
Definition
| a negatively charged electron cloud surrounding a positively charged nucleus |
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Term
| Which total mass is the smallest? |
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Definition
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Term
| How do the energy and the most probable location of an electron in the third shell of an atom compare to the energy and the most probable location of an electron in the first shell of the same? |
|
Definition
| In the third shell, an electron has mor energy and is farther from the nucleus |
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Term
| What is the total number of protons in atom with the electron configuration 2-8-18-32-18-1? |
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Definition
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Term
| Compared to an atom of hydrogen in the ground state, an atom of hydrogen in the excited has? |
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Definition
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Term
| What is the total number of electrons in the outrmost shell of a phosphorus atom in the ground state? |
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Definition
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Term
| Which statement best dscribes the mucleus of an aluminum atom? |
|
Definition
| It has a charge of +13 and is surrounded by a total of 13 electrons |
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Term
| The atomic mass of an element is weighd average of the |
|
Definition
| atomic masses of the naturally occuring istotopes of that element |
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Term
| Which electron configuration represents an atom of aluminum in an excited state? |
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Definition
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Term
| A 100.00-gram sample of naturally occuring boron contains 19.78 grams of boron-10 (atomic - 10.01 atomic mass units)and 80.22 grams of boron-11 (atomic = 11.01 atomic mass units). Which numerical setup can be used to determine atomic mass of naturally occuring boron? |
|
Definition
| (0.1978)(10.01) + (0.8022)(11.01) |
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Term
| What was concluded about the structure of the atom as th result of the gold foil experiment? |
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Definition
| A positively charged nucleus is surrounded by mostly empty space. |
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Term
| The nucleus of an atom of cobalt-58 contains... |
|
Definition
| 27 protons and 31 neutrons |
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Term
| The nucleus of atom of cobalt-58 contains... |
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Definition
| 27 protons and 31 neutrons |
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Term
| A proton has a charge that is opposite the charge of |
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Definition
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Term
| Which conclusion was a direct result of the gold foil experiment? |
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Definition
| An atom is mostly empty space with a dense, positively charged nucleus. |
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Term
| Which electron configuration represents an atom in an excited state? |
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Definition
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Term
| An electron has a charge of |
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Definition
| -1 and a smaller mass than a proton |
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Term
| What is the total number of neutrons in an atom of an element that has a mass number of 19 and atomic number of 9? |
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Definition
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Term
| An electron in atom moves from th ground state to an excited state when the energy of electron |
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Definition
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Term
| Atoms of different isotops of the same element differ in their total numbr of |
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Definition
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Term
| What is the total charge of the nucleus of a carbon atom |
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Definition
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Term
| Which statement explains why sulfur is classified as a Group 16 element? |
|
Definition
| A sulfur atom has 6 valence electrons |
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Term
| How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorus |
|
Definition
| Sodium has a larger atomic radius and is more metallic |
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Term
| Which group on the Periodic Table of th Elements contains elements that react with oxygen to form compounds with the general formula X(v)2O |
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Definition
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Term
| Elements on the modern Periodic Table are arranged in order of increasing |
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Definition
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Term
| Which element is a metal that is in the liquid phase at STP |
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Definition
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Term
| Which two elements have the most similar chemical properties |
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Definition
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Term
| In the ground state, each atom of an element has two valence lectrons. This element has a lower first ionization energy than calcium. Wher is the element located on th Periodic Table? |
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Definition
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Term
| Based on Reference Table S, which of the following atoms requirs the least energy for the removal of the most loosely, bound electron |
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Definition
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Term
| All atoms of a given element must contain the same number of |
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Definition
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Term
| Which brittle, nonconducting solid at 25 degrees celcius |
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Definition
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Term
| An atom of helium-4 differs from an atom of lithium-7 in that the atom of helium-4 has |
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Definition
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Term
| Antimony is classified as a |
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Definition
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Term
| Which list consists of element that have the most similar chemical properties? |
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Definition
|
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Term
| This question may require the use of the "Reference Tables for Physical Setting/Chemistry. At STP, an element that is a brittle solid and a poor conductor of heat and electricity could have an atomic number of ? |
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Definition
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Term
| The carbon atoms in graphite and the carbon atoms in diamond have different |
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Definition
|
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Term
| Which of these elements has physical and chemical properties most similar to silicon (Si)? |
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Definition
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|
Term
| What is the total number of protons in the nucleus of an atom of potassium-42? |
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Definition
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|
Term
| As the elements in Group 17 are considered in order of increasing atomic number , the chemical reactivity of each successive element |
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Definition
|
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Term
| Compared to the nonmetals in Period 2 , the metals in Period 2 generally have larger |
|
Definition
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|
Term
| Which of the following Group 2 elements has the lowest first ionization energy? |
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Definition
|
|
Term
| In Period 3 , from left to right in order , each successive element will |
|
Definition
| increase in number of protons |
|
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Term
| Which element is a solid at STP? |
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Definition
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|
Term
| In which group of the Periodic Table do most of the elements exhibit both positive and negative oxidation states? |
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Definition
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Term
| The element in Period 4 and Group 1 of the Periodic Table would be classified as a |
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Definition
|
|
Term
| Which set of symbols represents atoms with valence electrons in the same electron shell? |
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Definition
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Term
| A metal, M m forms an oxide compound with the general formula M(v)2O. In which group on the Periodic Table could metal M be found? |
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Definition
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Term
| Which trend appear as the elements in Period 3 are considered from left to right? |
|
Definition
| Metallic character decreases, and electronegativity increases. |
|
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Term
| What is a property of most metals? |
|
Definition
| They tend to lose electrons easily when bonding. |
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Term
| Which element is malleable and can conduct electricity in the solid phase? |
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Definition
|
|
Term
| The elements located in the lower left corner of the Periodic table are classified as |
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Definition
|
|
Term
| Which statement describes a chemical property of Iron? |
|
Definition
| Iron combines with oxygen to form rust. |
|
|
Term
| Which element is a noble gas? |
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Definition
|
|
Term
| Which element has both metallic and nonmetallic properties? |
|
Definition
|
|
Term
| Which isotopic notation identifies a metalloid that is matched with the corresponding number of protons in each of its atoms? |
|
Definition
|
|
Term
| The elements on the Periodic Table are arranged in order of increasing |
|
Definition
|
|
Term
| Which element had chemical properties that are most similar to those of calcium? |
|
Definition
|
|
Term
| Lithium and potassium have similar chemical properties because the atoms of both elements have the same |
|
Definition
| number of valence electrons |
|
|
Term
| What is the total number of valence electrons in an atom of sulfur in the ground state? |
|
Definition
|
|
Term
| When an atom loses one or more electrons, this atom becomes |
|
Definition
| A positive ion with a radius smaller than the radius of this atom |
|
|
Term
| Which two characteristics are associated with metals? |
|
Definition
| low first ionization energy and low electronegativity |
|
|
Term
| Which substance can not be decomposed by ordinary chemical means? |
|
Definition
|
|
Term
| Which statement describes a chemical property of iron? |
|
Definition
| Iron combines with oxygen to form rust |
|
|
Term
| What is a property of most metals? |
|
Definition
| They tend to lose electrons easily when bonding |
|
|
Term
| At STP , which element is brittle and not a conductor of electricity? |
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Definition
|
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Term
|
Definition
|
|
Term
| Which element is classified as a non metal? |
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Definition
|
|
Term
| At STP an element that is a brittle solid and a poor conductor of heat and electricity could have an atomic number of? |
|
Definition
|
|
Term
| Which element is a noble gas? |
|
Definition
|
|
Term
| Which substance can not be decomposed by a chemical change? |
|
Definition
|
|
Term
| Which group in the Periodic Table contains elements that are all monatomic gases at STP? |
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Definition
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|
Term
| Which element has both metallic and non metallic properties? |
|
Definition
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|
Term
| At standard pressure, which element has a melting point higher than standard temperature? |
|
Definition
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|
Term
| According to the Reference Table N , which pair of isotopes spontaneously decays? |
|
Definition
|
|
Term
| Which of these elements has the lowest melting point? |
|
Definition
|
|
Term
| The elements on the Periodic table are arranged in order of increasing |
|
Definition
|
|
Term
| Which element has chemical properties that are similar to those of calcium? |
|
Definition
|
|
Term
| Lithium and potassium have similar chemical properties because the atoms of both elements have the same |
|
Definition
| number of valence electrons |
|
|
Term
| An atom of argon rarely bonds to an atom of another element because an argon atom had |
|
Definition
|
|
Term
| What is the total number of valence electrons in an atom of sulfur in the ground state? |
|
Definition
|
|
Term
| Which trends are observed as each of the elements within Group 15 on the Periodic Table is considered in order from top to bottom? |
|
Definition
| Their metallic properties increase and atomic Radii increase. |
|
|
Term
| Atoms of which element have the greatest tendency to gain electrons? |
|
Definition
|
|
Term
| The strength of an atom's attraction for the electrons in a chemical bond is the atom's |
|
Definition
|
|
Term
| As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius , the ionization energy of each element successive element generally |
|
Definition
|
|
Term
| How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorus? |
|
Definition
| Sodium has a larger atomic radius and is more metallic |
|
|
Term
| Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number? |
|
Definition
| The atomic radius decreases, and the first ionization energy generally increases. |
|
|
Term
| Which period 4 element has the most metallic properties? |
|
Definition
|
|
Term
| As the elements in Period 2 of the Periodic Table are considered in succession from left to right there is a decrease in atomic radius with increasing atomic number. This may best be explained by the fact that the |
|
Definition
| number of protons increases , and the number of shells of electrons remains the same. |
|
|
Term
| As the atoms in Period 3 of the Periodic Table are considered from left to right , the atoms generally show |
|
Definition
| a decrease in radius and an increase in ionization energy |
|
|
Term
| Based on Reference Table S , atoms of which of these elements have the strongest attraction for the electrons in a chemical bond? |
|
Definition
|
|
Term
| Which phase change results in the release of energy? |
|
Definition
| Exothermic , Cooling Curve |
|
|
Term
| Which terms is defined as a measure of the average kinetic energy of the particles in a sample? |
|
Definition
|
|
Term
| At which temperature would atoms of a He(g) sample have the greatest average kinetic energy? |
|
Definition
|
|
Term
| Two samples of gold that have different temperatures are placed in contact with one another. Heat will flow spontaneously from a sample of gold at 60 Degrees Celsius to a sample of Gold that has a temperature of |
|
Definition
|
|
Term
| At which Celsius temperature does lead change from a solid to a liquid? |
|
Definition
|
|
Term
| The Boiling Point of a liquid is the temperature at which the vapor pressure of the liquid is equal to the pressure on the surface of the liquid. What is the boiling point of propanone if the pressure on its surface is 48 kilopascals? Table H |
|
Definition
|
|
Term
| Which grouping of the three phases of bromine is listed in order from left to right for increasing distance between bromine molecules? |
|
Definition
|
|
Term
| A sample of oxygen gas sealed in container X. A sample of hydrogen gas is sealed in container Z. Both samples have the same volume, temperature and pressure. Which statement is true? |
|
Definition
| Containers X and Z both contain the same number of gas molecules. |
|
|
Term
| Which statement describes a chemical property of the element magnesium? |
|
Definition
| Magnesium reacts with an acid |
|
|
Term
| Which statement best describes the shape and volume of an aluminum cylinder at STP? |
|
Definition
| It has a definite shape and a definite volume. |
|
|
Term
| Which process is a chemical change? |
|
Definition
|
|
Term
| Which statement describes a chemical property of oxygen? |
|
Definition
| Oxygen can combine with a metal to produce a compound. |
|
|
Term
| Which physical changes are endothermic? |
|
Definition
|
|
Term
| Which set of procedures and observation indicated a chemical change? |
|
Definition
| A cool , shiny metal is added to water in a beaker and rapid bubbling occurs. |
|
|
Term
| The temperature of a sample of water changes from 10 degrees Celsius to 20 degrees Celsius when the water absorbs 420 Joules of hear. What is the mass of the sample? |
|
Definition
|
|
Term
| In which process does a solid change directly into a vapor? |
|
Definition
|
|
Term
| The temperature of 100. grams of water changes from 16.0 Degrees Celsius to 20.0 Degrees Celsius. What is the total number of Joules of heat energy absorbed by the water? |
|
Definition
|
|
Term
| How much energy is required to vaporize 10.00 grams of water at its boiling point? |
|
Definition
|
|
Term
| Which intermolecular force of attraction accounts for the relatively high boiling point of water? |
|
Definition
|
|
Term
| Which liquid has the highest vapor pressure at 75 Degrees celsius ? |
|
Definition
|
|
Term
| Which substance has the lowest vapor pressure at 75 degrees Celsius ? |
|
Definition
|
|
Term
| At standard pressure , a certain compound has a boiling point and is insoluble in water. At STP, this compound most likely exists as |
|
Definition
|
|
Term
| A dilute, aqueos potassium nitrate solution is best classifies as |
|
Definition
|
|
Term
| Bronze contains 90 to 95% copper and 5 to 10% tin. Because these percentages can vary , bronze is classified as |
|
Definition
|
|
Term
| A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolves. Which statement best describes the resulting mixture? |
|
Definition
| The mixture is homogeneous and cannot be separated by filtration. |
|
|
Term
| When a mixture of water sand and salt is filtered, what passes through the filter paper? |
|
Definition
|
|
Term
| Which property makes it possible to separate the oxygen and the nitrogen from a sample of liquefied air? |
|
Definition
|
|
Term
| At Room temperature a mixture of sand and water can be separated by |
|
Definition
|
|
Term
| Compared to a 2.0 M aqueous solution of NaCl at 1 atmosphere, a 3.0 M aqueous solution of NaCl at 1 atmosphere has a |
|
Definition
| higher boiling point and a lower freezing point |
|
|
Term
| Compared to the freezing point of 1.0 M KCl(aq) at standard pressure, the freezing point of 1.0M CaCl(v)2 (aq) at standard pressure is |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| Homogeneous of heterogeneous |
|
|
Term
| Elements and compounds are |
|
Definition
|
|
Term
| A substance that can be broken down into simpler substances is |
|
Definition
|
|
Term
| Which of the following cannot be decomposed by chemical means |
|
Definition
|
|
Term
| A compound differs from an element in that a compound |
|
Definition
| Can be decomposed by chemical reaction |
|
|
Term
| A substance that is composed only of identical atoms is classified as |
|
Definition
|
|
Term
| Each particle contained in hydrogen gas is made up of two identical hydrogen atoms chemically joined together. Hydrogen is |
|
Definition
|
|
Term
| Which of the following material is a pure substance |
|
Definition
|
|
Term
| Which of the following is a mixture |
|
Definition
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Term
|
Definition
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Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| Which of the following is a mixture ? |
|
Definition
|
|
Term
| Which of the following is a mixture? |
|
Definition
|
|
Term
|
Definition
|
|
Term
| Which statement describes a chemical property of hydrogen gas? |
|
Definition
| Hydrogen gas burns in air. |
|
|
Term
| An aqueous solution fo sodium chloride is best classified as a |
|
Definition
|
|
Term
| Which of the following is a physical property? |
|
Definition
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Term
| A solid melts gradually between 85 degrees celsius and 95 degrees celsius to give a milky , oily liquid, When a laser beam shines through the liquid the path of the beam is clearly visible. The milky liquid is likely to be: |
|
Definition
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|
Term
| A sample of unknown composition was tested in a laboratory. The sample could not be decomposed by physical or chemical means. On the basis of these results the laboratory reported that the unknown sample was most likely |
|
Definition
|
|
Term
| Smoke is an example of an |
|
Definition
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|
Term
| Which process increases the potential energy of the particles of a sample? |
|
Definition
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Term
| Two solid samples each contain sulfur, oxygen and sodium, only. These samples have the same color , melting point , density , and reaction with an aqueous barium chloride solution. It can be concluded that the two samples are the same |
|
Definition
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|
Term
| Which transfer of energy occurs when ice cubes are placed in water that has a temperature of 45 degrees celsius? |
|
Definition
| Thermal energy is transferred from the water to the ice. |
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|
Term
| A sample is prepared by completely dissolving 10.0 grams of NaCl in 1.0 liter of H20. Which classification best describes this sample? |
|
Definition
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|
Term
| Which statement describes what occurs as two atoms of bromine combine to become a molecule of bromine? |
|
Definition
| Energy is released as bond is formed. |
|
|
Term
| Which formulas represent two polar molecules? |
|
Definition
|
|
Term
| What is the total number of valence electrons in a sulfide ion in the ground state? |
|
Definition
|
|
Term
| Which formula represents an ionic compound? |
|
Definition
|
|
Term
An unknown substance , liquid X, is tested in the laboratory. The Chemical and physical test results are listed below.
-Nonconductor of electricity
-Insoluble in water
-Soluble in hexane
-Low melting point as a solid
-Combustion produces only CO(v)2 and H(v)2O
Based on these results , a student should conclude that liquid X is |
|
Definition
|
|
Term
| The degree of polarity of a chemical bond in a molecule of a compound can be predicted by determining the difference in the |
|
Definition
| electronegativities of the bonded atoms in a molecule of the compound |
|
|
Term
| Based on electronegativity values, which type of elements tends to have the greatest attraction for electrons in a bond? |
|
Definition
|
|
Term
| What is the total number of pairs of electrons shared in a molecule of N(v)2? |
|
Definition
|
|
Term
| Which formula represents an ionic compound? |
|
Definition
|
|
Term
| Which characteristic is a property of molecular substances? |
|
Definition
|
|
Term
| Which substance is correctly paired with its type of bonding? |
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Definition
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|
Term
| Which compound contains only covalent bonds? |
|
Definition
|
|
Term
| Based on intermolecular forces, which of these substances would have highest boiling point? |
|
Definition
|
|
Term
| Which type of bonding is found in all molecular substances? |
|
Definition
|
|
Term
| Which substance contains bonds that involved the transfer of electrons from one atom to another? |
|
Definition
|
|
Term
| Which type of bond is formed when electrons are transferred from one atom to another? |
|
Definition
|
|
Term
| What occurs when an atom of chlorine forms a chloride ion? |
|
Definition
| The chlorine atom gains an electron and its radius becomes larger. |
|
|
Term
| As a bond between a hydrogen atom and sulfur atom is formed, electrons are |
|
Definition
| shared to form a covalent bond |
|
|
Term
| When ionic bonds are formed, metallic atoms tend to |
|
Definition
| lose electrons and become positive ions |
|
|
Term
| What occurs when an atom of chlorine and an atom of hydrogen become a molecule of hydrogen chloride? |
|
Definition
| A chemical bond is formed and energy is released. |
|
|
Term
| As two chlorine atoms combine to form a molecule, energy is |
|
Definition
|
|
Term
| What is conserved during a chemical reaction? |
|
Definition
|
|
Term
| Which symbol represents a particle that has the same total number of electrons as S^2-? |
|
Definition
|
|
Term
| Which electrons are represented by all of the dots? |
|
Definition
| the carbon and hydrogen valence electrons |
|
|
Term
| Based on your Reference Tables, the atoms of which of these elements have the strongest attraction for electrons in chemical bond? |
|
Definition
|
|
Term
| If the electronegativtity difference between the elements in compound NaX is 2.1, what is the element X? |
|
Definition
|
|
Term
| What occurs when an atom loses an electron? |
|
Definition
| The atoms's radius decreases and the atom becomes a positive ion. |
|
|
Term
| As a chlorine atom becomes a negative ion , the atom |
|
Definition
| gains an electron and its radius increases |
|
|
Term
| A substance that does not conduct electricity as a solid but does conduct electricity when melted is most likely classified as |
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Definition
|
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Term
|
Definition
|
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Term
|
Definition
|
|
Term
| a molecular compound is another name for |
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Definition
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|
Term
| A molecular compound never |
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Definition
|
|
Term
| Ionic compounds in (aq) solution |
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Definition
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Term
|
Definition
|
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Term
|
Definition
|
|
Term
| Which of the following solids has the highest melting point? |
|
Definition
|
|
Term
| What is total number of electrons shared in a double covalent bond between two atoms? |
|
Definition
|
|
Term
| Which type of bonding is found in all molecular substances? |
|
Definition
|
|
Term
| Which statement correctly describes diamond and graphite , which are different forms of solid carbon ? |
|
Definition
| They differ in their molecular structure and properties |
|
|
Term
| Which characteristics is a property of molecular substances? |
|
Definition
|
|
Term
| Conductivity in a metal results from the metal atoms having |
|
Definition
| highly mobile electrons in the valence shell |
|
|
Term
| Which substance contains metallic bonds? |
|
Definition
|
|
Term
| The high electrical conductivity of metals is primarily due to |
|
Definition
|
|
Term
| Silicon dioxide (SiO(sub2)) and diamonds are best described as |
|
Definition
| network solids with covalent bonding |
|
|
Term
| The bonds between hydrogen and oxygen in a water molecule are classified as |
|
Definition
|
|
Term
| Which type of molecule CF(sub4)? |
|
Definition
| nonpolar , with a symmetrical distribution of charge? |
|
|
Term
| Which formula represents a nonpolar molecule? |
|
Definition
|
|
Term
| At STP , fluorine is a gas and iodine is a solid. This observation can be explained by the fact that fluorine has |
|
Definition
| weaker intermolecular forces of attraction than iodine |
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Term
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Definition
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Definition
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Definition
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Definition
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Definition
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Definition
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Definition
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Definition
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Definition
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|
