Chemistry Chapter 5 Test

14a. Which elements are metalloids?

(semi-conducting elements) - B, Si, Ge, As, Sb, Te.

8b. List four of their characteristics properties.

- have a silvery appearance - combine vigorously with nonmetals - reactive - soft enough to be cut with a knife.

31. Identify the most - and least - electronegative groups of elements in the periodic table.

Group 17 & 1

12a. What types of elements make up the p block?

Nonmetals, metalloids, metals, and halogens.

7a. What information is provided by the specific block location of an element?

The type of sub level being filled in successive elements of that block.

17. Write the noble-gas notation for the electrons configuration of each of the following elements, and indicate the period in which each belongs. a. Li b. O *c. Cu d. Br e. Sn

a. [He] 2s^1 b. [He] 2s^2 2p^4 *(exception) c. [Ar] 4s^2 3d^9 = 3d^10 4s^1 d. [Ar] 3d^10 4s^2 4p^5 e. [Kr] 4d^10 5s^2 5p^2

29. For each of the following groups, indicate whether electrons are more likely to be lost or gained in compound formation and give the number of such electrons typically involved. a. Group 1 b. Group 2 c. Group 13 d. Group 16 e. Group 17 f. Group 18

a. lost, 1. b. lost, 2. c. lost, 3. d. gained, 2 e. gained, 1 f. neither lost nor gained, 0.

25b. Explain the basis for each trend.

across a period, the increasing nuclear charge attracts electrons in the same energy level more strongly and makes them more difficult to remove. down a group, the electrons to be removed from each successive element are farther from the nucleus in increasingly higher energy levels and are thus more easily removed.

24b. ionization

any process that results in the formation of an ion.

11. What name is sometimes used to refer to the entire set of d-block elements?

transition metals.

25a. How do the first ionization energies of main-group elements vary across a period and down a group?

they increase across a period and decrease down a group.

4a. How do the electron configurations within the same group of elements compare?

(they are the same) they share similar chemical properties. They also have the same valence electron configurations.

10b. How do the group numbers of those groups relate to the number of outer s and d electrons?

*the group number equals the sum of the outer s and d electrons.* The group number tells how many electrons there are in the outer shells; group 1 has 1 electron, group 2 has 2 electrons, and so forth

13b. List three of their characteristics properties.

- most reactive nonmetals. - react vigorously with most metals - form compounds.

14b. Describe their characteristic properties.

- mostly brittle solids w/ some properties of metals and non-metals. - have electrical conductivity intermediate between that of metals and nonmetals.

7b. Identify, by number, the groups located within each of the four block areas.

S block: groups 1 & 2. P block: groups 13-18, except helium. D block: groups 3-12. F block: wedged between groups 3 and 4 in the sixth and seventh periods.

5. What determines the length of each period in the periodic table?

The length of each period is determined by the number of electrons that can occupy the sublevels being filled in that period.

12b. How do the properties of the p-block metals compare with those of the metals in the s and d blocks?

The p block metals are generaly harder and more dense then the s block metals but softer and less dense than the d- block metals.

6. What is the relationship between the electron configuration of an element and the period in which that element appears in the periodic table?

The period of an element can be determined from an element's electron configuration. *An elements period corresponds to its highest occupied main energy level.*

9b. How do their characteristics properties compare with those of the alkali metals?

They are harder, denser, and stronger than alkali metals. And they have higher melting points. Less reactive than alkali metals.

21. Identify the block, period, group, group name (where appropriate), element name, element type, and reactivity for the elements with the following electron configuration. (Hint: See Sample Problem D.) a. [Ne] 3s^2 3p^1 b. [Ar] 3d^10 4s^2 4p^6 c. [Kr] 4d^10 5s^1 d. [Xe] 4f^1 5d^1 6s^2

a. Block: p. Period: 3. Group: 3. Group name: none. Element name: Aluminum. Type: Metal. Reactivity: b. Block: p. Period: 4. Group: 18. Group name: Noble Gases. Element name: Krypton. Type: Nonmetal. Reactivity: c. Block: d. Period: 5. Group: 11. Group name: Transition metals. Element name: Silver. Type: Metal. Reactivity: d. Block: d. Period: 6. Group: none. Group name: Transition metal. Element name: Cerium. Type: Metal. Reactivity:

18. Without looking at the periodic table, identify the period, block, and group in which the elements with the following electron configurations are located. (Hint: See Sample Problem A.) a. [Ne] 3s^2 3p^4 b. [Kr] 4d^10 5s^2 5p^2 c. [Xe] 4f^14 5d^10 6s^2 6p^5

a. Period: 3. Block: p. Group: 16. b. Period: 5. Block: p. Group: 14. c. Period: 6. Block: p. Group: 17

28a. What are valence electrons?

valence electron are atomic electrons available to be lost, gained, or shared in the formation of chemical compounds.

28b. Where are such electrons located?

valence electrons are located in an atom's outermost energy level.

22c. Explain this trend.

As electrons are added to s and p sublevels in the same main energy level, the increasing positive charge of the nucleus pulls electrons closer to the nucleus, resulting in decreasing atomic radii.

27b. How does the size of each compare with the size of the neutral atom from which it is formed?

Cations are always smaller than the atoms from which they are formed; anions are always larger.

10a. Write the group configurations notation for each d-block group.

D1s2 d2s2 d3s2 d5s1 d5s2 d6s2 d7s2 d8s2 d10s1 d10s2

8a. Which elements are designated as the alkali metals?

Elements of group 1. lithium, sodium, potassium, rubidium, cesium and francium.

9a. Which elements are designated as the alkaline-earth metals?

Elements of group 2. beryllium, magnesium, calcium, strontium, barium, and radium.

4b. Why are the noble gases relatively unreactive?

Noble gases are reactively unreactive because they neither want to gain or lose electrons. *they have a completely filled outer level.* this means they have completely filled s and p sublevels which gives them a "stable octet." electrons in their outer level.

27a. Distinguish between a cation and an anion.

a cation is a positive ion, and an anion is a negative ion.

24a. ion

a charged atom or a charged group of bonded atoms.

22a. What is meant by atomic radius?

a one half the distance between the nuclei of two bonded identical atoms.

20. Without looking at the periodic table, write the expected outer electron configuration for each of the following elements. (Hint: See Sample Problem C.) a. Group 7, fourth period. b. Group 3, fifth period. c. Group 12, sixth period.

a. 3d^5 4s^2. Mn, Manganese. b. 4d^1 5s^2. Y, Yttrium. *c. 4f^14 5d^10 6s^2. Hg, Mercury.

19. Based on the information given below, give the group, period, block, and identity of each element described. (Hint: See Sample Problem B.) a. [He] 2s^2 b. [Ne] 3s^1 c. [Kr] 5s^2 d. [Ar] 4s^2 e. [Ar] 3d^5 4s^1

a. Group: 2. Period: 2. Block: s. Element: Be, Beryllium. b. Group: 1. Period: 3. Block: s. Element: Na, Sodium. c. Group: 2. Period: 5. Block: s. Element: Sr, Strontium. d. Group: 2. Period: 4. Block: s. Element: Ca, Calcium. e. Group: 6. Period: 4. Block: d. Element: Cr, Chromium.

16b. What trends can be observed across the various periods within the main-group elements?

decrease in atomic size, increase in ionization energy, increase in electron affinity, decrease in cationic size, decrease in anionic size increase in electronegativity.

23b. Explain this trend.

down a group, the outer electrons of each element occupy comparable sublevels in successively higher main energy levels farther from the nucleus.

26b. What signs are associated with electrons affinity values, and what is the significance of each sign?

electron affinity values are either negative or positive. a negative sign indicated that energy is given off; a positive sign indicates that energy is taken in.

13a. Which elements are designated as the halogens?

elements of group 17. fluorine, chlorine, bromine, iodine, and astatine.

30b. Why is flourine special in terms of electronegativity?

fluorine is the most electronegativity element and is arbitrarily assigned an electronegativity of 4.0 The values for all other elements are assigned in relation to this value.

15. Which elements make up the f block in the periodic table?

inner transition elements: lanthanides and actinides.

30a. What is electronegativity?

is the ability of an atom in a chemical compound to attract electrons from other atoms.

24d. second ionization energy

the energy required to remove an electron from a 1+ ion.

24c. first ionization energy

the energy required to remove one electron from a neutral atom of an element.

26a. What is electron affinity?

the energy taken in or given off when an electron is added to an atom.

16a. What are main-group elements?

the p block elements together with the s block elements.

22b. What trend is observed among the atomic radii of main-group elements across a period?

they decrease.

23a. What trend is observed among the atomic radii of main-group elements down a group?

they generally increase.