Mock Exam Which elements have a single s electron in their outermost shell? a. Na, Al, Ar b. Cl, I, Br c. Cl, O, N d.

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Mervin McDaniel
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1 Mock Exam 2 1. What is Aufbau s principle? a. Electrons have a negative one charge b. Electrons have opposite spins c. Electrons fill the lowest-energy atomic orbitals of a ground-state first d. The radius of an atom depends on its placement on the periodic table 2. What is Hund s rule? a. Any set of degenerate orbitals, each orbital must contain one electron before any orbital in the set can accept a second electron b. Electrons fill the lowest-energy atomic orbitals of a ground-state first c. Electrons have a negative one charge d. Electron emit energy called a photon when they jump from a lower energy level to a higher one 3. Heisenberg uncertainty principle states that a. the position of an electron can be known only if the momentum is known b. the position and momentum of an electron cannot both be precisely know at the same time c. the momentum of an electron can only be known if the position is known d. the position and momentum of an electron can never be known 4. Which elements have a single s electron in their outermost shell? a. Na, Al, Ar b. Cl, I, Br c. Cl, O, N d. Na, Cr, Au 5. Which element s outermost shells are filled? a. Halogens b. Alkane earth c. Transition metals d. Noble gasses 6. What is a node? a. It s when the amplitude of a wave is equal to zero b. It s when the amplitude of a wave is equal to one c. It s the distance from crest to crest on a wave d. It s when a wave is has its highest amplitude

2 7. What is order of waves from greatest to least amount of energy? a. ROYGBIV b. Radio, Microwave, Infrared, Visible, Ultraviolet, X-rays, Gamma rays c. Gamma rays, X-rays, Ultraviolet, Visible, Infrared, Microwave, Radio d. X-rays, Ultraviolet, Radio, Microwave, Gamma rays, Infrared, Visible 8. What is the ground state of on atom or ion? a. It s when all electrons of an atom or ion are in the lowest possible energy b. It s when all protons of an atom or ion are in the lowest possible energy c. It all the electrons that aren t valance electrons d. It s when electrons jump energy levels 9. What is an ionic bond? a. It s a bond that results from a sharing of electrons b. It s a bond that results in attraction of ions c. It s a bond that results from a non-metal and a non-metal only d. None of the above 10. What is a covalent bond? a. It s a bond that results from a sharing of electrons b. It s a bond that results in attraction of ions c. It s a bond formed from on atom stealing another atoms electrons d. None of the above 11. Electronegativity increases a. down and to the left b. up and to the left c. down and to the right d. up and to the left 12. An unequal sharing of electrons between atoms is called what? a. Polar covalent bond b. Polar ionic bond c. Non-polar covalent bond d. Non-polar ionic bond

3 13. Which group of atoms has two valence electrons? a. Group 1 b. Group 2 c. Group 15 d. Group Which of the following substances has the most negative lattice? a. KCl b. TiO2 c. Ba Cl2 d. KI 15. What is the role of the Roman numeral in the names of compounds formed by transition metals? a. To show the number of atoms of that element there are b. To show the number of valence electron that the transition metal has c. To show the charge of the transition metal d. To show the charge of what the transition metal is bonded to 16. What is the covalent name for water? a. H2O b. Dihydrogen monoxide c. Two hydrogen one oxygen d. Monohydrogen dioxide 17. What is the charge of group 17 anions? a. +1 b. -1 c. +2 d What is the charge of group 2 cations? a. +1 b. -1 c. +2 d. -2

4 19. All transition metals have a charge of? a. +2 b. -2 c. +/-2 d. None of the above 20. All of the memorized polyatomic ions have a charge of? a. +/-1 b. +/-2 c. A and B d. None of the above Number of atoms Prefix Ion Name Ion Name NH4 + NO2 - Hydroxide Nitrate CN - ClO - Acetate Chlorite SO4 2- ClO4 - Hydrogen sulfate Carbonate S2O3 2- HCO3 - Phosphate HPO4 2- Cr2O7 2- Dihydrogen phosphate SCN - MnO4 - Cyanate Oxalate Chromate

5 Naming Covalent Bonds phosphorus triiodide dihydrogen monoxide diphosphorous pentoxide NF3 H2O N2O5 Naming Ionic Bonds molybdenum sulfate platinum (II) sulfide ammonium sulfate CdSO Cu(NO2)2 Fe(HCO3)2

6 Lewis Dot Structure PBr3 N2H2 CH3OH CH4 CCl2F2 H2O

7 Electron Configuration As Cl Mo Al N Xe Orbital Diagrams Br: S: Co: K:

8 Equation Problems What is the frequency of a radiation wave that has a wavelength of 660 nm? What is the energy of a radiation wave with a wavelength of 714 nm? What is the energy it takes to excite an electron from n=2 to n=4? Potassium has a work function of 3.68x10-19 J. What frequency of radiation can be used to make energy? What are the formal charges on each individual atom, as well as the overall formal charge, on CH3COOH?

Ionic Bonding (Ch.7) Covalent Bonding (Ch.8) Metallic Bonding

Ionic Bonding (Ch.7) Covalent Bonding (Ch.8) Metallic Bonding Unit 3: Chemical Bonding Outline Ionic Bonding (Ch.7) Valence electrons Positive and negative ions and transition metal ions Ionic bonding: Charge on compounds Ionic compounds characteristics Writing ionic