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The energy that results from the breaking or formation of chemical bonds is
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"In any chemical or physical process, energy is neither created nor destroyed" is a statement of the
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Chemistry1SemTest
| Question | Answer |
|---|---|
| The energy that results from the breaking or formation of chemical bonds is | chemical energy |
| "In any chemical or physical process, energy is neither created nor destroyed" is a statement of the | law of conservation of energy |
| The specific heat of a given substance | is unique to that substance |
| A temperature that is equivalent to 20 degrees Celsius | 293 K |
| For every investigation, the scientific method | is a logical set of procedures |
| The reason for organizing, analyzing, and classifying data is | to find relationships among the data |
| There are ______ variables represented in the weather graphs | four |
| Of the items depicted, only _______ is not a model. | figure d |
| A plausible explanation of a body of observed natural phenomena is a scientific | theory |
| The matter diagram represent a(n) | theory |
| A theory is an accepted explanation of an observed phenomenon until | repeated data and observation conflict with the theory |
| Poor precision in scientific measurement may arise from | both human error and the limitations of the measuring instrument |
| precision pertains to all of the following except | closeness of a measurement to an accepted value |
| Five darts strike near the center of the target. Whoever threw the darts is | both accurate and precise |
| A chemist who frequently carries out a complex experiment is likely to have high | precision |
| When applied to scientific measurements, the word accuracy and precision | have distinctly different meanings |
| When determining the number of significant digits in a measurement, | all nonzero digits are significant |
| To two significant figures, the measurement 0.0255 g should be reported as | 0.026 g |
| In division and multiplication, the answer must not have more significant figures than the | number in the calculation with the fewest significant figures |
| The number of significant figures in the measurement 170.040 km is | 6 |
| The measurement that has been expressed to four significant figures is | 30.00 mm |
| What is the density of 37.72 g of matter whose volume is 6.80 cm ^3 | 5.55 g/cm^3 |
| The dimensions of a rectangular solid are measured to be 1.27 cm, 1.3 cm, and 2.5 cm. The volume should be recorded as | 4.1 cm^3 |
| Three samples of 0.12g, 1.8g, and 0.562 g are mixed together. The combined mass of all three samples, expressed to the correct number of significant figures, should be recorded as | 2.5 g |
| Expressed in scientific notation, 0.0930 m is | 9.3 ' 10^-2 m. |
| When 6.02 ' 10^23 is multiplied by 9.1 ' 10^/31 the product is | 5.5' 10^-7 |
| The law of conservation of mass follows from the concept that | atoms are indivisible |
| The composition of the two oxides of lead, PbO and PbO2, are explained by | law of multiple proportions |
| Who first proposed an atomic theory based on scientific knowledge? | John Dalton |
| According to Dalton's atomic theory, atoms | of each element are identical in size, mass, and other properites. |
| Which of the following is NOT part of Dalton's atomic theory? | The number of protons in an atom is its atomic number. |
| The law of definite proportions | was explained by Dalton's atomic theory. |
| In a cathode tube, electrical current passes from one electrode, the _______, to the oppositely charged electrode. | cathode |
| Experiments with cathode rays led to the discovery of the | electron |
| Who explained the behavior of positively charged particles being deflected from a metal foil as the nucleus? | Ernest Rutherford |
| In a gold foil experiment, most of the particles fired at the foil | passed through the foil |
| The gold foil experiment led to the discovery of the | nucleus |
| What did Rutherford conclude about the structure of the atom> | An atom contains a small, dense, positively charged central region |
| A nuclear particle that has about the same mass as a proton, but with no electrical charge is called a(n) | neutron |
| Which part of an atom has a mass approximately equal to 1/2000 of the mass of a common hydrogen atom? | electron |
| The mass of a neutron is | about the same as that of a proton |
| The nucleus of most atoms is composed of | tightly packed protons and neutrons |
| Protons and neutrons strongly attract when they | are very close together |
| An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is | 27 |
| Isotopes are atoms of the same element that have different | masses |
| Atoms of the same element that have different masses are called | isotopes |
| Isotopes of an element contain different numbers of | neutrons |
| When the light from excited atoms of an element is passed through a prism, the distinct colored lines produced are called | line-emission spectra |
| Bohr's theory helped explain why | excited hydrogen gas gives off certain colors of light |
| According to Bohr's theory, an excited atom would | radiate energy |
| If electrons in an atom have the lowest possible energies, the electrons are in their | ground states |
| For an electron in an atom to change from the ground state to an excited state | energy must be absorded |
| Most of the volume of an atom is occupied by the | electron cloud |
| The main energy levels of an atom are indicated by the | principal quantum numbers |
| The letter designations for the first four sublevels, with the number of electrons that can be accommodated in each sublevel are | s2; p6; d10; and f14 |
| The number of obitals for the d sublevel is | 5 |
| The statement that an electron occupies the lowest available energy orbital is | that aufbau principle |
| "Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin" is a statment of | Hund's rule |
| The statement that no more than two electrons in the same atom can occupy a single orbital is | the Pauli exclusion principle |
| Which of the following rules requires that each of the p orbitals at a particular energy level receive one electron before any of them can have two electrons? | Hund's rule |
| Two electrons in the 1s orbital must have different spin quantum numbers to satisfy | the Pauli exclusion principle |
| The sequence in which energy sublevels are filled is specific by | aufbau principle |
| Which is the ground-state electron configuration for 24 Cr? | [Ar] 4s^1 3d^5 |
| The carbon-12 atom is assigned a relative mass of exactly | 12 amu |
| The abbreviation for atomic mass unit is | amu |
| The idea of arranging the elements in a table according to their chemical and physical properties is attributed to | Newlands |
| From gaps in his table, Mendeleev predicted the existence of several element and their | properties |
| Mendeleev is credited with developing the first successful | periodic table |
| The principle that states that the physical and chemical properties of the elements are periodic functions of their atomic numbers is | the periodic law |
| The period law states that | the physical and chemical properties of the elements are functions of their atomic numbers |
| Elements in a group or column in the periodic table can be expected to have similar | properties |
| The atomic number of sodium, the first element in Period 3, is 11. The atomic number of the second element in this period is | 12 |
| Elements in a group have similar | electron configurations |
| An element that has an electron configuration of [He] 2s^2 2p^3 is in Period _______ of the periodic table | 2 |
| An element that has an electron of [Ne] 3s^2 3p^3 is in Group ____ of the periodic table. | 15 |
| To which group of the periodic table do lithium and potassium belong to | alkali metals |
| To which group of the periodic table do fluorine and chlorine belong to? | halogens |
| The outer electron configuration of an alkali metal has | 1 electron in the s orbital |
| The element in Group 17 are known by what name? | halogens |
| Transition elements are found in which of the following group(s) of the periodic table? | Groups 3-12 |
| An element that has four electrons in its outermost s orbital is a member of what group in the periodic table | Group 5 |
| Moving from left to right across _______, electrons are being added to the 4f orbitals. | the lanthanides |
| A property of all the actinides is that they are | Both members of Period 7 and radioactive |
| A metal is called malleable if it | can be hammered into sheets |
| A solution of two or more metals is | an alloy |
| Trends in the properties of elements in a group or period can be explained in terms of | electron configuration |
| The effect of inner electrons on the attraction between the nucleus and the outer electrons of an atom is called | electron shielding |
| Trends in the periodic table indicate that the element with the greatest ionization energy is in which of the following periods and groups? | Period 1, Group 18 |
| One method of measuring the size of an atom involves calculating a value that is ______ the distance between the nuclei of two bonded atoms | half |
| Going down a group in the periodic table, electron shielding generally causes the effective nuclear charge to | decrease |
| Going across a period in the periodic table, electron shielding generally has little effect. As a result, the effective nuclear charge | increases |
| Which is the best reason that the atomic radius generally increases with atomic number in each group of elements? | The number of energy levels increases |
| For the alkaline-earth metals with the smallest radii have the | highest ionization energies |
| Trends in the periodic table indicate that an element in which of the following periods and groups will have the smallest anion (negative ion) radius? | Period 7, Group 1 |
| Electron affinity tends to | increase across a period and decrease down a group |
| The process that changes one element into another different element is called | transmutation |
| Which of the following electron configurations belongs to an element that is NOT chemically reactive | 1s2 2s2 2p6 3s2 3p6 |
| In the compound sodium fluoride, NaF, the sodium atom loses one electron and the fluorine atoms gains one electron to form ions that have electron configurations similar to | neon |
| In many compound, atoms of the main-group elements form ions so that the number of electrons in the outermost energy levels of each ion is | 8 |
| The electron configuration of nitrogen is 1s2 2s2 2p3. How many more electrons does nitrogen need to have an electron configuration similar to neon | 3 |
| Atoms of copper and iron | tend to form cations |
| An anion | is an ion with a negative charge |
| When the octet rule is satisfied, the outermost _______ are filled | s and p orbitals |
| The elements of the _____ groups satisfy the octet rule without forming compounds | noble gas |
| Once an atom has full s and p orbitals in its outermost energy level, | it has a stable octet and is unreactive |
| An ion and its parent atom have the same | atomic number |
| The energy released when a salt is formed from gaseous ions is called the | lattice energy |
| The lattice energy is a measure of the | strength of an ionic bond |
| If the lattice energy of compound A is greater than that of compound B, | the bonds in compound A are stronger than the bonds in compound B |
| When ions are formed, | energy can be released or absorbed |
| When an electron is added to an atom, | energy is usually released |
| Which of the following is NOT a property of an ionic compound? | low boiling point |
| Compared with ionic compound, molecular compounds | have lower melting points |
| The melting points of ionic compound are higher than the melting points of molecular compounds because | attractive forces between ions are greater than the attractive forces between molecules |
| Because ions are more strongly attracted in an ionic compound than molecules are attracted in molecular compounds, the melting points of ionic compounds are | higher than the melting points of molecular compounds |
| Ionic compounds are brittle because the strong attractive forces | hold the layers in relatively fixed positions |
| In the NaCl crystal, each Na+ and Cl- ion has clustered around it ____ of the oppositely charged ions | 6 |
| In a crystal of an ionic compound, each cation is surrounded by | anions |
| A compound that has the same number of positive and negative charges is said to be | electroneutral |
| What is the ratio of cations to anions in a compound composed of sodium ions, Na+, and carbonate ions, Co3 (2-charge) | 2 to 1 |
| The indium (II) ion and indium (III) ion | have charges of 2+ and 3+, respectively |
| What is the metallic ion in the compound CuCl2 | Cu 2+ |
| What is the formula for the compound formed by calcium ions, Ca 2+, and chloride ions, Cl-? | CaCl2 |
| The chemical formula for an ionic compound represents the | simplest ration of ions that results in an electrically neutral compound |
| The symbol HCO3 - represents a | polyatomic ion |
| A comparison of calcium sulfate and calcium sulfite shows that | both have a monatomic cation and polyatomic anion |
| What is the formula for the compound formed by lead (II) ions and chromate ions, CrO4 2-? | PbCrO4 |
| What is the formula for the compound formed by aluminum (III) and the sulfate ion, SO4 2-? | Sl2(SO4)3 |
| What is the formula for the compound formed by tin (IV) and the chromate ion, CrO4 (2- charge) | Sn(CrO4)2 |
| What is the formula for the compound formed by the barium ion, Ba (2+), and the hydroxide ion, OH (-1)? | Ba(OH)2 |
| Name the compound Ni(ClO3)2 | nickel chlorate |
| Name the compound Zn3(PO4)2 | zinc phosphate |
| Name the compound Hg2(NO3)2 | mercury (1) nitrate |
| Name the compound KClO3 | potassium chlorate |
| Name the compound Fe(NO2)2 | iron (II) nitrite |
| Name the compound CuCO3 | copper (II) carbonate |
| What is the name of Sn3(PO4)4 | tin(IV) phosphate |
| The name of a polyatomic ion that contains hydrogen begins with the term | hydrogen |
| The electrons involved in the formation of a covalent bond are | valence electrons |
| The chemical bond formed when two atoms share one or more pairs of electrons is a(n) | covalent bond |
| If two covalently bonded atoms move farther that a distance of the bond length, the potential energy of the atoms | increases |
| A covalent bond forms when the attraction between two atoms is balanced by repulsion and the potential energy is | at a minimum |
| Which of the following compounds most likely has the least bond energy? | I2; I-I bond length = 266 pm |
| A nonpolar covalent bond is most likely to form between two elements that have a difference in electronegativity values of | 0.1 |
| An ionic bond is most likely to form between two elements that have a difference in electronegativity values of | 3.0 |
| A polar covalent bond is most likely to form between two elements that have a difference in electronegativity values of | 1.5 |
| Which of the following molecular formulas show that polar nature of the HBr molecule? | H+ Br- |
| Which of the following substances most likely has the lowest boiling point? | Cl2 |
| The correct Lewis structure for the oxygen atom has | two pairs of valence electrons and two single valence electrons |
| The correct Lewis structure for the boron atom has | three single valence electrons |
| The correct Lewis structure for a Group 18 atom has | four pairs of valence electrons |
| The correct Lewis structure for a fluorine atom in a molecule of F2 shows | All of the above |
| To draw the Lewis structure of the polyatomic ion, ClO3 - , you would have to _______ those in the structures of Cl, O, O, and O | add one electron to |
| In a double bond, two atoms share a total of ______ electrons | four |
| The correct Lewis structure for a molecule of the compound C2H2 contains | one triple bond |
| To indicate resonance, a ______ is placed between a molecule's resonance structure | double headed arrow |
| Which of the following number of atoms can form a tetrahedral molecule | five |
| According to VSEPR theory, which of the following shapes is possible for a molecule with the molecular formula AB2 | both linear and bent |
| According to the VSEPR theory, which of the following shaoes is possible for a molecule with the molecular formula of AB3 | both trigonal planar and trigonal pyrimidal |
| According to the VSEPR theory, a molecule with the molecular formul of A2 is | linear in shape |
| According to VSEPR theory, the molecular shape of CO2 is classified as | linear |
| According to the VSEPR theory, the molecular shape of H2O is classified as | bent |
| Iodine monochloride, ICl, has a higher boiling point than bromine, Br2, partly because ICl is a(n) | polar molecular substance |
| The number of atoms in a mole of any pure substance is called | Avogadro's number |
| What can be said about 1 mol Ag and 1 mol Au? | They contain the same number of atoms |
| An Avogadro's number of any element is equivalent to | 6.022 ' 10^23 particles |
| If 0.500 mol a Na+ combines with 0.500 mol of Cl- to form NaCl, how many formula units of NaCl are present | 3.01 ' 10^23 |
| Using a periodic table, what is the average atomic mass of zinc | 65.39 amu |
| The atomic mass of hydrogen is 1.008 amu. The reason that this value is not a whole number is that | hydrogen has more than one isotope |
| A chemical formula includes the symbols of the elements in the compound and subscripts that indicate | the number of atoms or ions of each type |
| How many atoms of fluorine are in a molecule of carbon tetraflouride, CF4? | 4 |
| Changing a subscript in a correctly written chemical formula | changes the formula so that it no longer represents that compound |
| A formula that shows the simplest whole-number ration of the atoms in a compound is the | empirical formula |
| The molar mass of an element is the mass of one | mole of the element |
| To determine the molar mass of an element, one must know the element's | average atomic mass |
| What is the molar mass of magnesium? | 24.305 g |
| What is the empirical formula for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen | KClO3 |
| What is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen? | P2O5 |
| What is the empirical formula for a compound that is 53.3% O and 46.7% Si? | SiO2 |
| A compound contains 64 g of O and 4g of H. What is the empirical formula for this compound | HO |
| A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula for this compound? | CF4 |
| What is the empirical formula for a compound that is 36.1% Ca and 63.9% Cl | CaCl2 |
| A compound contains 27.3 g of C and 72.7 g of O. What is the empirical formula for this compound? | CO2 |
| To find the molecular formula from the empirical formula, one must determine the compound's | formula mass |
| A molecular compound has the empirical formula XY3. Which of the following is a possible molecular formula | X2Y6 |
| The molecular formula for vitamin C is C6H8O6. What is the empirical formula? | C3H4O3 |
| A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula? | N2O4 |
| What is the percentage composition of CF4? | 13.6% C, 86.4% F |
| What is the percentage composition of CuCl2 | 47.267% Cu, 52.733% Cl |
| The percentage of sulfur in SO2 is about 50%. What is the percentage of oxygen in this compound? | 50% |
| What is the percentage of OH- in Ca(OH)2 | 45.9% |
| The temperature of 323 K is equivalent to | 50 degrees Celsius |
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