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Chemistry Test 1
| Question | Answer |
|---|---|
| The wave model of light does not explain | the photoelectric effect |
| A line spectrum is produced when an electron moves from one energy level | to a lower energy level |
| Because excited hydrogen atoms always produce the same line-emission spectrum, scientists concluded that hydrogen | released photons of only certain energies |
| For an electron in an atom to change from the ground state to an excited state, | energy must be absorbed |
| According to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus | in specific allowed orbits |
| The change of an atom from an excited state to the ground state always requires | emission of electromagnetic radiation |
| The region outside the nucleus where and electron can most probably be found is the | electron cloud |
| The size and shape of an electron cloud are most closely related to the electron's | energy |
| The spin quantum number indicates that the number of possible spin states for an electron in an orbital is | 2 |
| The set of orbitals that are dumbbell shaped and directed along the x,y, and z axes are called | p orbitals |
| A spherical electron cloud surrounding an atomic nucleus would best represent | an s orbital |
| The major difference between a 1s orbital and a 2s orbital is that | the 2s orbital is at a higher energy level |
| The letter designations for the first four sublevels with the maximum number of electrons that can be accommodated in each sublevel are | s:2, p:6, d:10, f:14 |
| The number of possible different orbital shapes for the third energy level is | 3 |
| The number of orbitals for the d sublevel is | 5 |
| For the f sublevel, the number of orbitals is | 7 |
| The total number of orbitals that can exist at the second main energy level is | 4 |
| How many orbitals can exist at the third main energy level? | 9 |
| How many electrons are needed to completely fill the fourth energy level | 32 |
| If the third energy level contains 15 electrons, how many more could it possible hold? | 3 |
| The statement that no two electrons in the same atom can have the same four quantum number is | the Pauli exclusion principle |
| Two electrons in the 1s orbital must have different spin quantum numbers to satisfy | the Pauli exclusion principle |
| The Aufbau principle states that an electron | must be added to elements and ions in a very specific order |
| The atomic sublevel with the next highest energy after 4p is | 5s |
| What lists atomic orbitals in the correct order they are filled according to the Aufbau principle? | 1s 2s 2p 3s 3p 4s 3d 4p 5s |
| The electron notation for aluminum (atomic number 13) is | 1s^2 2s^2 2p^6 3s^2 3p^1 |
| The number of electrons in the highest energy level of the argon atom (atomic number 18) is | 8 |
| The atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element in this group is | 11 |
| How much greater is the atomic number of the fourth element in groups 1,2, and 18 than the preceding element? | 18 |
| Krypton, atomic number 36, is the fourth element in Group 18. What is the atomic number of xenon, the fifth element in Group 18? | 54 |
| Barium, atomic number 36, is the fifth element in Group 2. What is the atomic number of radium, the next element in Group 2? | 88 |
| For elements in groups 1,2, and 18, the increase in atomic number for successive elements follows the pattern 8,8,18,___,32. What number completes the pattern? | 18 |
| The electron configuration of cesium, atomic number 55, is [Xe] 6s^1. In what period is cesium? | 6 |
| Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel? | 16 |
| For groups 13 through 18, the total number of electrons in the highest occupied level equals the group number | minus 10 |
| Which block in the periodic table contains the alkali metals? | S |
| Compared to alkali metals, the alkaline-earth metals | are less reactive |
| A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called | electronegativity |
| One-half the distance between the nuclei of identical atoms that are bonded together is called the | atomic radius |
| What is removed when the ionization energy is supplied to an atom of an element? | an electron |
| When an electron is acquired by a neutral atom, the energy change is called | electron affinity |
| The element that has the greatest electronegativity is | fluorine |
| In a row in the periodic table, as the atomic number increases, the atomic radius generally | decreases |
| Within a group of elements, as the atomic number increases, the atomic radius | increases |
| In the alkaline-earth group, atoms with the smallest radii | have the highest ionization energies |
| As you move down Group 14 in the periodic table from carbon through lead, atomic radii | generally increase |
| As you move from left to right in Period 4 from gallium through bromine, atomic radii | generally decrease |
| The electrons available to be lost, gained, or shared when atoms form compounds are called | valence electrons |
| Across a period, ionization energies of d-block elements generally | increase |
| Which groups in the main group have lower electronegativity than d-block elements? | groups 1 and 2 |
| A bond that is less than 5% ionic is considered | nonpolar covalent |
| The pair of elements that forms a bond with the least ionic character is | Mg and Cl |
| The B-F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is | ionic |
| What shows the types and numbers of atoms joined in a single molecule of a molecular compound? | molecular formula |
| The electron configuration of nitrogen is 1s^2 2s^2 2p^3. How many more electrons does nitrogen need to satisfy the octet rule? | 3 |
| Multiple covalent bonds may occur in atoms that contain carbon, nitrogen, or | oxygen |
| The substance whose Lewis structure shows three covalent bonds is | NH3 |
| Compared with energies of neutral atoms, a crystal lattice has | lower potential energy |
| Compared with ionic compounds, molecular compounds | have lower melting points |
| How many extra electrons are in the Lewis structure of the phosphate ion, PO4^3- | 3 |
| Compared with nonmetals, the number of valence electrons in metals is generally | smaller |
| According to VSEPR theory, an AB2 molecule is | linear |
| According to VSEPR theory, the shape of an AB3 molecule is | trigonal-planar |
| According to VSEPR theory, the structure of the ammonia molecule, NH3 is | trigonal-pyramidal |
| Use VSEPR theory to predict the shape of the magnesium hydride molecule, MgH2. | linear |
| Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, Cl4. | tetrahedral |
| Use VSEPR theory to predict the shape of carbon dioxide, CO2. | linear |
| What is the formula for zinc fluoride? | ZnF2 |
| What is the formula for the compound formed by lead(II) ions and chromate ions? | PbCrO4 |
| What is the formula for aluminum sulfate? | Al2(SO4)3 |
Created by:
MistyCoy