Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Gen Chem (2)
| Question | Answer |
|---|---|
| What is the difference between a group and a period on the periodic table? | A group is a column — elements share the same number of valence electrons. A period is a row — elements share the same number of electron shells. |
| What are the names of the major groups on the periodic table? | Group 1 (excl. H): Alkali metals Group 2: Alkaline earth metals Groups 3–12: Transition metals Groups 13–16: Includes metalloids Group 17: Halogens Group 18: Noble gases |
| What are inner transition metals, and where are their valence electrons? | The two bottom rows of the periodic table. Period 6 = lanthanides; Period 7 = actinides. Their valence electrons are in the f-orbital (vs. d-orbital for transition metals). Most prominent oxidation state is +3 (transition metals = +2). |
| What are post-transition metals and where are they located? | Post-transition metals sit between the transition metals and metalloids in groups 13–15 (e.g., Al, Ga, In, Sn, Tl, Pb, Bi). They are metals but are softer and have lower melting points than transition metals. Tend to have fixed, lower oxidation states. |
| What are the 7 diatomic atoms? | Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Clorine, Bromine. Mnemonic: Have No Fear Of Ice Cold Beer |
| How do metals and non-metals differ in appearance? | Metals are malleable and lustrous; non-metals are brittle and dull. |
| How do metals and non-metals differ in conductivity? | Metals are good conductors of electricity and heat; non-metals are poor conductors. |
| What type of oxides do metals and non-metals form? | Metals form basic oxides; non-metals form acidic oxides. |
| How do metals and non-metals differ in electron behavior? | Metals lose electrons to form cations; non-metals gain electrons to form anions. |
| What is the physical state of metals and non-metals at room temperature? | Metals are solid at room temperature, except mercury (Hg), which is liquid. Non-metals are gas or solid, except bromine (Br), which is liquid. |
| How do melting and boiling points differ between metals and non-metals? | Metals generally have high melting and boiling points; non-metals generally have low melting and boiling points. |
| How does metallic character change across the periodic table? | Increases going right to left across a period, and increases going down a group. |
| Define atomic radius and state its trend. | Half the distance between the nuclei of two identical bonded atoms. Increases going right → left across a period and down a group. |
| Why does atomic radius increase going left and going down? | Going left: fewer protons → weaker nuclear pull → shells spread out. Going down: more electron shells → electrons farther from nucleus. |
| Define Zeff and give the formula. | The net positive charge felt by a valence electron after accounting for shielding by inner electrons. Zeff = Z − S (Z = protons, S = shielding/non-valence electrons) |
| How does Zeff change across the periodic table? | Increases left → right across a period (more protons, no new shells). Increases slightly going down a group (nuclear charge increase outweighs added shielding). |
| What is an isoelectronic series, and how do you rank radius within one? | Atoms/ions with the same number of electrons but different protons. More protons = stronger pull = smaller radius. Anions > neutral atoms > cations in size. |
| How does forming an anion or cation affect atomic radius? | Anions (gain e⁻) → more e⁻-e⁻ repulsion → larger radius. Cations (lose e⁻) → less repulsion → smaller radius. |
| Define ionization energy and state its trend. | Energy needed to remove an electron from an atom. Increases going left → right across a period and up a group. |
| How do successive ionization energies behave, and when is there a big jump? | Each successive ionization energy is higher than the last. A huge jump occurs when removal would disturb a stable, full electron shell (e.g., Na's 2nd ionization: 496 → 4562 kJ/mol). |
| What are the two exceptions to the ionization energy trend? | Group 2 > Group 13 in the same period (e.g., Be > B) — filled s-orbital gives extra stability. Group 15 > Group 16 in the same period (e.g., N > O) — half-filled p-orbital gives extra stability. |
| Define electron affinity and state its trend. | Energy released when an electron is added to a neutral atom. Increases going left → right across a period and up a group. |
| What are the three exceptions to the electron affinity trend? | Group 2: filled s-orbitals → very low EA Group 15: half-filled p-orbitals → lower EA than Group 14 Noble gases: filled shells → negligible EA |
| Define electronegativity and state its trend. | An atom's ability to attract a bonding electron pair. Increases left → right across a period and up a group. Most electronegative element: Fluorine. Noble gases have no electronegativity value. |
| In which directions does atomic radius increase on the periodic table? | Increases going right → left across a period; increases going down a group. |
| In which directions does effective nuclear charge (Zeff) increase on the periodic table? | Increases going left → right across a period; increases slightly going down a group. |
| In which directions does ionization energy increase on the periodic table? | Increases going left → right across a period; increases going up a group. |
| In which directions does electron affinity increase on the periodic table? | Increases going left → right across a period; increases going up a group. |
| In which directions does electronegativity increase on the periodic table? | Increases going left → right across a period; increases going up a group. |
| In which directions does metallic character increase on the periodic table? | Increases going right → left across a period; increases going down a group. |
Created by:
smurtab