Honors Chemistry: Unit 3

Of the following elements, which one would have the largest electronegativity energy: Iodine (I, atomic #53), Chlorine (Cl, atomic #17), Bromine (Br, atomic #35), Fluorine (F, atomic #9) - Fluorine(F, atomic #9) Of the following elements, which one would have the largest ionization energy: Potassium (K, atomic #19), Cesium (Cs, atomic #55), Sodium (Na, atomic #11), Hydrogen (H, atomic #1) - Hydrogen (H, atomic #1) Of the following elements, which one would have the largest radius: Cesium (Cs, atomic #55), Hydrogen (H, atomic #1), Potassium (K, atomic #19), Sodium (Na, atomic #11) - Cesium (Cs, atomic #55) Anions have a ______________ charge and are ______________ than the atoms from which they formed. - negative/larger The elements with the largest atomic radii are found in the: - lower left-hand corner of the periodic table As one moves from down ( ↓ ) a group on the periodic table, the ionization energy of the elements encountered tends to: - decrease The elements with the smallest atomic radii are found in the: - upper right-hand corner of the periodic table The least electronegative elements are the: - alkali metals Generally speaking, the group of elements with the highest first ionization energy is: - group 18 The measure of the attraction that an atom has for electrons involved in chemical bonds is known as: - electronegativity A horizontal row ( → ) of elements on the periodic table may also be referred to as a: - period/series The energy required to remove an electron from an atom is known as: - ionization energy The most active metals are located in the: - lower left hand corner of the periodic table As one moves from down ( ↓ ) a group on the periodic table, the atomic radius of the elements encountered tends to: - increase As one moves from left to right ( → ) within a period across the periodic table, the atomic radius of the elements encountered tends to: - decrease As one moves from down ( ↓ ) a group on the periodic table, the electronegativity of the elements encountered tends to: - decrease As one moves from left to right ( → ) within a period across the periodic table, the ionization energy of the elements encountered tends to: - increase A vertical column ( ↓ ) of elements on the periodic table may also be referred to as a: - family/group As one moves from left to right ( → ) within a period across the periodic table, the electronegativity of the elements encountered tends to: - increase Of the following elements, which one would have the smallest radius: Bromine (Br, atomic #35), Iodine (I, atomic #53), Fluorine (F, atomic #9), Chlorine (Cl, atomic #17) - Fluorine (F, atomic #9) Of the following elements, which one would have the smallest ionization energy: Boron (B, atomic #5), Neon (Ne, atomic #10), Nitrogen (N, atomic #7), Lithium (Li, atomic #3) - Lithium (Li, atomic #3) Cations have a ______________ charge and are ______________ than the atoms from which they formed. - positive/smaller Of the following elements, which one would have the largest radius: Lithium (Li, atomic #3), Neon (Ne, atomic #10), Nitrogen (N, atomic #7), Boron (B, atomic #5) - Lithium (Li, atomic #3) Of the following elements, which one would have the smallest radius: Nitrogen (N, atomic #7), Neon (Ne, atomic #10), Boron (B, atomic #5), Lithium (Li, atomic #3) - Neon (Ne, atomic #10) Which group of elements will have half-filled p sublevels? boron group carbon group nitrogen group oxygen group - nitrogen group What is the definition of ionization energy? -Energy needed to attract an electron into an atom -Energy needed to remove the outermost electron from an atom -Energy released when the nucleus is split -Energy leftover after the valence level is filled with electrons. - Energy needed to remove the outermost electron from an atom Which of the following atoms has the highest ionization energy? barium radon gold lead - radon Which of the following statements is true regarding atomic radius? -The radius increases as you move from left to right on the table. -The radius decreases as you move from left to right on the table. -All atoms in the same period have the same radius -All atoms in the same family have the same radius. - The radius decreases as you move from left to right on the table. Which family of elements all have two valence electrons? -noble gases -halogens -carbon group -alkaline earth metals -alkali metals - alkaline earth metals Why do the radius of atoms decrease within a period as you move left to right? There are fewer electrons There are more protons pulling the electrons tighter There are fewer energy levels There are more neutrons attracting the electrons - There are more protons pulling the electrons tighter Which atom will increase in size when forming its most common ion? fluorine sodium aluminum magnesium - fluorine Which of the following atoms has the highest electronegativity? magnesium silicon argon sulfur - sulfur Which family of atoms below would be the most reactive? halogens nitrogen group oxygen group noble gases - halogens Which of the following atoms has the lowest ionization energy? silver zinc aluminum carbon - silver Which family of atoms will form ions with a +2 charge? halogens nitrogen group alkali metals alkaline earth metals - alkaline earth metals What charge would an aluminum atom typically form? +1 +2 +3 -3 -2 -1 - +3 Which element listed below would be the most reactive? lithium radium titanium cobalt - lithium Which of the following elements has 7 valence electrons? oxygen bromine argon potassium - bromine Which of the following atoms has the largest radius? arsenic calcium iron zinc - calcium Why do atoms get smaller as you go from left to right across a period on the periodic table? - There are more protons in the nucleus as you move from left to right within a period. However, there are an identical number of energy levels. Therefore, more protons pull the energy level tighter toward the nucleus, making the atoms smaller. What is ionization energy? - The energy needed to remove the outermost electron from an atom. List at least four characteristics of a wave, and describe each. - Crest- peak of each wave Trough- bottom of each wave Wavelength- distance between two consecutive crests or troughs Frequency- number of waves that pass a point per second Amplitude- distance from the middle of the wave (rest position) to the crest Period- time it takes for one wave to pass a point. What is a quantum of energy? Why do we not notice these? - Energy travels in small pieces or bundles. These bundles are called a quantum. They are so small, we cannot notice them. The idea what is a quantum(small particle of energy) energy can act like a particle when traveling at high speeds and very small size. Why do elements each produce a unique line spectrum? - As electrons absorb energy, they become "excited" and move to higher energy levels. When they release this energy, we see it as a specific wavelength of light(a line on the line spectrum). Each possible movement from a higher energy to lower energy produces a different line. Describe the wave-mechanical model of the atom. - The nucleus of the atom is small, dense, and positively charged. The locations of the electrons are not known exactly, since the act of measuring the location of the electron makes it moves. Thus, electrons are said to be found in orbitals, which are areas where are electrons are "most likely" found. Explain the photoelectric effect. - Certain wavelengths of light (ones with high enough energy) are able to knock electrons free when it strikes a metal. When the main group elements (s and p block) have a full set of electrons, what is the charge for each family? - Alkali metals +1 Alkaline earth metals +2 Boron group +3 Carbon group +/- 4 Nitrogen group -3 Oxygen group -2 Halogens -1 Noble gases 0 Why do noble gases not form ions? Why are the noble gases not reactive? - They already possess a full valence level, therefore they do not need to gain, lose, or share any electrons. How do valence electrons determine how an atom forms chemical bonds? - Atom will gain, lose, or share electrons in a chemical bond in order to acquire a full valence (outer energy) level.