AP Chem Ch 7

Each set of lettered choices below refers to the numbered statements immediately following it. Select the one lettered choice that best fits each statement. A choice may be used once, more than once, or not at all in each set. (A) Cs (B) Ag (C) Pb (D) Br (E) Se Has the largest atomic radius

(A) Cs

Steel is an alloy containing FeFe atoms and C atoms. Which of the following diagrams best represents the particle-level structure of steel?

(choice with big Fe and small C) C is in the second period and has two electron shells, whereas Fe is in the fourth period and has four electron shells; thus C atoms are smaller than Fe atoms. The diagram shows how the smaller C atoms occupy the spaces (interstices) between the larger Fe atoms in an interstitial alloy.

Copper atoms and zinc atoms have the same atomic radius, 135 picometers. Based on this information, which of the following diagrams best represents an alloy containing only copper and zinc atoms?

(choice with uniform diff colored dots) Being the same size, copper atoms and zinc atoms would form a substitutional alloy in which the atoms substitute for one another in a lattice of positive cores immersed in a sea of electrons.

What does Pauli exclusion principle state ? - states that each electron occupies the lowest energy orbital available - states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins - states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

- states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins

What does Hund's rule states ? - states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals - states that each electron occupies the lowest energy orbital available - states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins

- states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

How many electrons can the d sublevel hold? 8 10 2 4

10

The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is 3 6 8 10

10

How many electrons does Si contain? (click to see image) 14 28 2 4

14

What is the maximum number of electrons that an f orbital can have? 11 electrons 14 electrons 13 electrons 12 electrons

14 electrons

How many electrons can the third energy level hold? 2 18 8 0

18

What do you start all electron configurations with? 1s2 1d10 1f14 1p6

1s2

An element has an atomic number of 11. Which of the following represents its correct electron configuration? 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s11 1s2 2s2 2p6 3s1 1s2 2s2 3p6 3s1

1s2 2s2 2p6 3s1

Identify the Electron Configuration for Aluminum (Al) 1s2 2s2 2p6 3s2 3p1 1s2 2s2 2p6 3s2 3p3 1s2 2s2 2p6 3s2 4p1

1s2 2s2 2p6 3s2 3p1

Which electron configuration belongs to Chlorine (Cl)? 1s2 2s2 2p6 3s2 3p5 1s2 2s2 2p6 3s2 3p6 1s2 2s2 2p6 3s2 3p7

1s2 2s2 2p6 3s2 3p5

What electron configuration matches an oxygen atom? 1s22s22p63s2, 3p64s23d104p5 1s22s22p4 1s22s22p6 1s22s22p63s23p64s23d1

1s22s22p4

How many electrons can the first energy level hold? 1 2 8 0

2

Identify the error in 1s2 2s1 2p6 3s2. 1s2 2s1 2p6 3s2

2s1

How many p orbitals are there in a sublevel? 2 1 4 3

3

The potential energy of a system of two atoms as a function of their internuclear distance is shown in the diagram above. Which of the following is true regarding the forces between the atoms when their internuclear distance is x? A The attractive and repulsive forces are balanced, so the atoms will maintain an average internuclear distance x. B There is a net repulsive force pushing the atoms apart, so the atoms will move further apart. C There is a net attractive force pulling the atoms together, so the atoms will move closer together. D It cannot be determined whether the forces between atoms are balanced, attractive, or repulsive, because the diagram shows only the potential energy

A The attractive and repulsive forces are balanced, so the atoms will maintain an average internuclear distance x.

Which of the following represents an electron configuration that corresponds to the valence electrons of an element for which there is an especially large jump between the second and third ionization energies? (Note: n represents a principal quantum number equal to or greater than 2.) A ns2 B ns2np1 C ns2np2 D ns2np3

A ns2 The third ionization of this element would involve removing an electron that is closer to the nucleus (in the adjacent lower shell) than are the first two electrons. This would require much more energy than the removal of the first two electrons.

Consider atoms of the following elements. Assume that the atoms are in the ground state. The atom that contains exactly two unpaired electrons A. S B. Ca C. Ga D. Sb E. Br

A. S

Electrons occupy orbitals of lowest energy first is part of what electron configuration rule? Hund's Rule Aufbau Principle Pauli Exclusion Principle

Aufbau Principle

Electrons are filled from the lowest energy orbitals to the higher energy orbitals. This refers to ______. Pauli - exclusion principle Aufbau principle Hund's rule Heisenberg principle

Aufbau principle

The complete photoelectron spectrum of an element is given above. Which of the following electron configurations is consistent with the spectrum? A 1s2 2s2 2p1 B 1s2 2s2 2p6 3s2 3p3 C 1s2 2s2 2p6 3s2 3p6 D 1s2 2s2 2p6 3s2 3p6 4s2 3d5

B 1s2 2s2 2p6 3s2 3p3 The leftmost peak in the spectrum has the highest energy and contains two electrons; this is the peak that corresponds to the 1s electrons. Moving to the right, the next peak is the 2s peak, then the 2p peak, and then the 3s peak. The last peak is the 3p peak, which contains only 3 electrons. The correct electron configuration 1s22s22p63s23p3.

First: 801 Second: 2430 Third: 3660 Fourth: 25000 Fifth: 32820 The first five ionization energies of a second-period element are listed in the table above. Which of the following correctly identifies the element and best explains the data in the table? A B, because it has five core electrons B B, because it has three valence electrons C N, because it has five valence electrons D N, because it has three electrons in the p sublevel

B B, because it has three valence electrons

Atoms of Mg combine with atoms of F to form a compound. Atoms of which of the following elements combine with atoms of F in the same ratio? A Li B Ba C Al D Cl E Ne

B Ba

Which of the following best helps to account for the fact that the F- ion is smaller than the O2- ion? A F- has a larger nuclear mass than O2- has. B F- has a larger nuclear charge than O2- has. C F- has more electrons than O2- has. D F- is more electronegative than O2- is. E F- is more polarizable than O2- is.

B F- has a larger nuclear charge than O2- has.

The melting point of MgO is higher than that of NaF. Explanations for this observation include which of the following? I. Mg2+ is more positively charged than Na+. II. O2- is more negatively charged than F-. III. The O2- ion is smaller than the F- ion. A II only B I and II only C I and III only D II and III only E I, II, and III

B I and II only

The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following? A Na has a greater density at standard conditions than Ne. B Na has a lower first ionization energy than Ne. C Na has a higher melting point than Ne. D Na has a higher neutron-to-proton ratio than Ne. E Na has fewer naturally occurring isotopes than Ne.

B Na has a lower first ionization energy than Ne.

The diagram above represents the photoelectric effect for a metal. When the metal surface is exposed to light with increasing frequency and energy of photons, electrons first begin to be ejected from the metal when the energy of the photons is 3.3×10−19J. Color Wavelength Red 647−760nm Orange 585−647nm Yellow 575−585nm Green 491−575nm Blue 424−491nm Violet 300−424nm Using the wavelength information provided above, what is the color of the light? A Red B Orange C Yellow D Blue

B Orange The color is orange since it corresponds to wavelengths in the range of 585−647nm. The wavelength λ of the light is 600nm, found from λ=cν=cEh=hcE=(6.6×10−34 J⋅s)(3.0×108 m/s)3.3×10−19 J=6.0×10−7m=600nm.

Which of the following shows the correct number of protons, neutrons, and electrons in a neutral cesium-134 atom? A Protons Neutrons Electrons 55 55 55 B Protons Neutrons Electrons 55 79 55 C Protons Neutrons Electrons 55 79 79 D Protons Neutrons Electrons 79 55 79 E Protons Neutrons Electrons 134 55 134

B Protons Neutrons Electrons 55 79 55

Which of the following can be inferred from the diagram above that shows the dependence of potential energy on the internuclear distance between two atoms? A The atoms form a bond with a bond length of 25pm. B The atoms form a bond with a bond length of 75pm. C The net force between the atoms is attractive at 25pm. D The net force between the atoms is attractive at 75pm.

B The atoms form a bond with a bond length of 75pm.

The elements C and Se have the same electronegativity value, 2.55. Which of the following claims about the compound that forms from C and Se is most likely to be true? A The carbon-to-selenium bond is unstable. B The carbon-to-selenium bond is nonpolar covalent. C The compound has the empirical formula CSe. D A molecule of the compound will have a partial negative charge on the carbon atom.

B The carbon-to-selenium bond is nonpolar covalent. The bonding in compounds between elements with the same (or only slightly different) electronegativity values will exhibit covalent bonding (that is, more or less equal sharing of electrons).

The complete photoelectron spectrum of a pure element is shown in the diagram above. If peaks 1 and 2 represent s sublevels, which of the following sublevels is represented by peak 3? A. s B. p C. d D. f

B. p

Why does electronegativity decrease as you go down a group? As you go down a group, the outer electrons are further away from the nucleus As you go down a group, the nucleus is less able to attract electrons in a bond Both of these None of these

Both of these

Which of the following is the ground-state electron configuration of the F− ion? A 1s2 2s2 2p4 B 1s2 2s2 2p5 C 1s2 2s2 2p6 D 1s2 2s2 2p6 3s2 3p6

C 1s2 2s2 2p6 Because of its −1 charge, the fluoride ion has 10 electrons, just like an Ne atom has.

Which of the following is the ground-state electron configuration of the F− ion? A 1s2 2s2 2p4 B 1s2 2s2 2p5 C 1s2 2s2 2p6 D 1s2 2s2 2p6 3s2 3p6

C 1s2 2s2 2p6 Correct. Because of its −1 charge, the fluoride ion has 10 electrons, just like an Ne atom has.

Which of the following best represents the ground-state electron configuration for an atom of selenium? A 1s2 2s2 2p6 3s2 3p3 B 1s2 2s2 2p6 3s2 3p4 C 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 D 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

C 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 Correct. This configuration follows the Aufbau principle and represents 34 electrons in total.

Which of the following best represents the ground-state electron configuration for an atom of selenium? A 1s2 2s2 2p6 3s2 3p3 1s2 2s2 2p6 3s2 3p3 B 1s2 2s2 2p6 3s2 3p4 1s2 2s2 2p6 3s2 3p4 C 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 D 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

C 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 This configuration follows the Aufbau principle and represents 34 electrons in total.

Which of the following best helps to explain why the value of ΔH° for the dissolving of CaF2 in water is positive? A CaF2(s) is insoluble in water. B CaF2(s) dissolves in water to form CaF2(aq) particles. C Ca2+ ions have very strong ion-ion interactions with F- ions in the crystal lattice. D Ca2+ ions have very strong ion-dipole interactions with water molecules in the solution.

C Ca2+ ions have very strong ion-ion interactions with F- ions in the crystal lattice.

Consider atoms of the following elements. Assume that the atoms are in the ground state. The atom that contains only one electron in the highest occupied energy sublevel A S B Ca C Ga D Sb E Br

C Ga

The complete photoelectron spectrum for an element is shown above. Which of the following observations would provide evidence that the spectrum is consistent with the atomic model of the element? A A neutral atom of the element contains exactly two electrons. B The element does not react with other elements to form compounds. C In its compounds, the element tends to form ions with a charge of +1. D In its compounds, the element tends to form ions with a charge of +3. (PES shows 1s2 2s1)

C In its compounds, the element tends to form ions with a charge of +1.

Two pure elements react to form a compound. One element is an alkali metal, X, and the other element is a halogen, Z. Which of the following is the most valid scientific claim that can be made about the compound? A It has the formula XZ2. B It does not dissolve in water. C It contains ionic bonds. D It contains covalent bonds.

C It contains ionic bonds. An alkali metal will readily lose an electron and a halogen will readily gain an electron to form an ionic compound with a 1:11:1 ratio of X+:Z−X+:Z− ions.

Which of the following correctly indicates whether the solid represented by the particulate model shown above conducts electricity and explains why or why not? A It conducts electricity because it is made of positive and negative ions. B It conducts electricity because it is made of particles of different sizes. C It does not conduct electricity because its ions cannot move freely within the solid. D It does not conduct electricity because there are small spaces between the particles.

C It does not conduct electricity because its ions cannot move freely within the solid. (In the solid state, the ions are held by strong coulombic forces in fixed positions within the lattice; thus they cannot move or migrate through the lattice.)

The lattice energy of a salt is related to the energy required to separate the ions. For which of the following pairs of ions is the energy that is required to separate the ions largest? (Assume that the distance between the ions in each pair is equal to the sum of the ionic radii.) A Na+(g) and Cl−(g) B Cs+(g) and Br−(g) C Mg2+(g) and O2−(g) D Ca2+(g) and O2−(g)

C Mg2+(g) and O2−(g)

All the chlorides of the alkaline earth metals have similar empirical formulas, as shown in the table above. Which of the following best helps to explain this observation? A Cl2(g) reacts with metal atoms to form strong, covalent double bonds. B Cl has a much greater electronegativity than any of the alkaline earth metals. C The two valence electrons of alkaline earth metal atoms are relatively easy to remove. D The radii of atoms of alkaline earth metals increase moving down the group from Be to Ra.

C The two valence electrons of alkaline earth metal atoms are relatively easy to remove. By easily losing their two valence electrons, the alkaline earth metal atoms react with chlorine atoms to form M2+ cations that combine in a 1-to-2 ratio with Cl− anions.

The table above shows the first ionization energy and atomic radius of several elements. Which of the following best helps to explain the deviation of the first ionization energy of oxygen from the overall trend? A The atomic radius of oxygen is greater than the atomic radius of fluorine. B The atomic radius of oxygen is less than the atomic radius of nitrogen. C There is repulsion between paired electrons in oxygen's 2p orbitals. D There is attraction between paired electrons in oxygen's 2p orbitals.

C There is repulsion between paired electrons in oxygen's 2p orbitals.

Which of the following best helps explain why the electronegativity of Cl is less than that of F? A The mass of the Cl atom is greater than the mass of the F atom. B The Cl nucleus contains more protons than the F nucleus contains. C When Cl and F form bonds with other atoms, the Cl bonding electrons are more shielded from the positive Cl nucleus than the F bonding electrons are shielded from the positive F nucleus. D Because Cl is larger than F, the repulsions among electrons in the valence shell of Cl are less than the repulsions among electrons in the valence shell of F.

C When Cl and F form bonds with other atoms, the Cl bonding electrons are more shielded from the positive Cl nucleus than the F bonding electrons are shielded from the positive F nucleus. Electronegativity is based on the ability of atoms participating in bonding to attract bonding electrons to themselves. The smaller size and lower amount of shielding in F cause it to be more electronegative than Cl.

A particle-level diagram of a metallic element is shown above. Typically, metals are both malleable and ductile. The best explanation for these properties is that the electrons involved in bonding among metal atoms are A unequally shared and form nondirectional bonds B unequally shared and form highly directional bonds C equally shared and form nondirectional bonds D equally shared and form highly directional bonds

C equally shared and form nondirectional bonds In metals, electrons are free to move as described by the electron sea model. Electrons are shared equally among atoms, and the structure is based on simple close-packed structures that contain no fixed directional bonds.

First: 580 Second: 1815 Third: 2740 Fourth: 11600 Fifth: 14800 The ionization energies for element X are listed in the table above. On the basis of the data, element X is most likely to be A. Na B. Mg C. Al D. Si E. P

C. Al

Which of the following ions has the same number of electrons as Br - ? A. Ca2+ B. K+ C. Sr2+ D. I- E. Cl-

C. Sr2+

Which of the following will have a lower ionization energy than Scandium (Sc)? Helium (He) Titanium (Ti) Calcium (Ca) Magnesium (Mg)

Calcium (Ca)

Which of the following ground-state electron configurations represents the atom that has the lowest first-ionization energy? A 1s2 2s1 B 1s2 2s2 2p2 C 1s2 2s2 2p6 D 1s2 2s2 2p6 3s1

D 1s2 2s2 2p6 3s1

Which of the following ground-state electron configurations represents the atom that has the lowest first-ionization energy? A 1s2 2s1 B 1s2 2s2 2p2 C 1s2 2s2 2p6 D 1s2 2s2 2p6 3s1

D 1s2 2s2 2p6 3s1 Correct. An electron in a 3s sublevel is farthest from the nucleus. Based on Coulomb's law, this weakens the attractive force between the electron and the nucleus, making it easier to remove.

Which of the following correctly identifies which has the higher first-ionization energy, Cl or Ar, and supplies the best justification? A Cl, because of its higher electronegativity B Cl, because of its higher electron affinity C Ar, because of its completely filled valence shell D Ar, because of its higher effective nuclear charge

D Ar, because of its higher effective nuclear charge

If Na reacts with chlorine to form NaCl, which of the following elements reacts with Na to form an ionic compound in a one-to-one ratio, and why? A K, because it is in the same group as Na. B Mg, because its mass is similar to that of Na. C Ar, because its mass is similar to that of Cl. D Br, because it has the same number of valence electrons as Cl.

D Br, because it has the same number of valence electrons as Cl. Br is in the same group as Cl and has the same number of valence electrons, namely 7. Like Cl, Br can accept an electron from Na to become a negatively charged ion (Br−). Thus, Br forms the compound NaBr, which is analogous to NaCl.

RbCl has a high boiling point. Which of the following compounds is also likely to have a high boiling point, and why? A NO, because its elements are in the same period of the periodic table. B ClF, because its elements are in the same group of the periodic table. C Cl2O, because its elements have similar electronegativities and it is a covalent compound. D CsCl, because its elements have very different electronegativities and it is an ionic compound.

D CsCl, because its elements have very different electronegativities and it is an ionic compound. Cs , like Rb, is an alkali metal. Thus it reacts with halogens, like Cl, in a 1:1 ratio to form an ionic compound. Ionic compounds have relatively high melting points and boiling points.

Which of the following represents a pair of isotopes? Atomic Number | Mass Number A I. 6 | 14 II. 7 | 14 B I. 6 | 7 II. 14 | 14 C I. 6 | 14 II. 14 | 28 D I. 7 | 13 II. 7 | 14 E I. 8 | 10 II. 16 | 20

D I. 7 | 13 II. 7 | 14

The photoelectron spectra above show the energy required to remove a 1s electron from a nitrogen atom and from an oxygen atom. Which of the following statements best accounts for the peak in the upper spectrum being to the right of the peak in the lower spectrum? A Nitrogen atoms have a half-filled p subshell. B There are more electron-electron repulsions in oxygen atoms than in nitrogen atoms. C Electrons in the p subshell of oxygen atoms provide more shielding than electrons in the p subshell of nitrogen atoms. D Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

D Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

Which of the following correctly compares periodic properties of two elements and provides an accurate explanation for that difference? A The first ionization energy of Al is greater than that of B because Al has a larger nuclear charge than B does. B The first ionization energy of F is greater than that of O because O has a higher electronegativity than F has. C The atomic radius of Ca is larger than that of Mg because the valence electrons in Mg experience more shielding than the valence electrons in Ca do. D The atomic radius of Cl is smaller than that of S because Cl has a larger nuclear charge than S does.

D The atomic radius of Cl is smaller than that of S because Cl has a larger nuclear charge than S does.

Which of the following scientific claims about the bond in the molecular compound HFHF is most likely to be true? A There is a partial negative charge on the HH atom. B Electrons are shared equally between the HH and FF atoms. C The bond is extremely weak. D The bond is highly polar.

D The bond is highly polar. Fluorine is the most electronegative element, and the difference between the electronegativities of HH and FF is relatively large, resulting in a bond that is highly polar.

The energy required to dissociate an ionic solid into gaseous ions (lattice energy) for the compounds NaFNaF and MgF2MgF2 is shown in the table above. On the basis of Coulomb's law, which of the following best helps to explain the large difference between the lattice energies of NaFNaF and MgF2MgF2 ? A The solubility of MgF2 is less than that of NaF. B The electronegativity of Mg is greater than that of Na. C The mass of the Mg cation is greater than that of the Na cation. D The charge of the Mg cation is larger than that of the Na cation.

D The charge of the MgMg cation is larger than that of the NaNa cation. The coulombic attractions between the MgMg cation and FF anions are stronger because of the +2+2 charge on MgMg as opposed to the +1+1 charge on NaNa. Stronger interionic attractions lead to a higher lattice energy.

The photoelectron spectrum for the element nitrogen is represented above. Which of the following best explains how the spectrum is consistent with the electron shell model of the atom? A The leftmost peak represents the valence electrons. B The two peaks at the right represent a total of three electrons. C The electrons in the 1s sublevel have the smallest binding energy. D The electrons in the 2p sublevel have the smallest binding energy.

D The electrons in the 2p sublevel have the smallest binding energy. Correct. The electrons in the 2p sublevel have the smallest binding energy because these electrons have the weakest attraction to the nucleus and are more easily removed from the atom.

Which of the following best helps to explain why Na(s) is more reactive with water than Mg(s) is? A Na(s) is softer than Mg(s). B The atomic mass of Na is less than that of Mg. C The Na+ ion has weaker Coulombic attraction to an anion than the Mg2+ ion has. D The first ionization energy of Na is less than that of Mg .

D The first ionization energy of Na is less than that of Mg . Ionization energy is the energy needed to remove an electron from an atom. When Na and Mg react with water, they lose electrons to become positive ions. The first ionization energy of Na is less than that of Mg, so Na loses an electron more easily than Mg does.

Which of the following best helps to explain why the electron affinity of Br has a greater magnitude than that of I? A Br has a lower electronegativity than I does. B Br has a lower ionization energy than I does. C An added electron would go into a new shell in Br but not in I. D There is a greater attraction between an added electron and the nucleus in Br than in I.

D There is a greater attraction between an added electron and the nucleus in Br than in I. Br has one less electron shell than I does, so, on average, an electron added to the outer shell of Br is closer to the nucleus and less shielded than an electron added to the outer shell of I.

Each set of lettered choices below refers to the numbered statements immediately following it. Select the one lettered choice that best fits each statement. A choice may be used once, more than once, or not at all in each set. (A) Cs (B) Ag (C) Pb (D) Br (E) Se Has the highest electronegativity

D. Br

The elements in which of the following have most nearly the same atomic radius? A Be, B, C, N B Ne, Ar, Kr, Xe C Mg, Ca, Sr, Ba D C, P, Se, I E Cr, Mn, Fe, Co

E Cr, Mn, Fe, Co

1s2 2s2 2p6 3s2 3p3 Atoms of an element, X, have the electronic configuration shown above. The compound most likely formed with magnesium, Mg, is A MgX B Mg2X C MgX2 D MgX3 E Mg3X2

E Mg3X2

Which of the following elements has the largest first ionization energy? A. Li B. Be C. B D. C E. N

E. N

What atom matches this electron configuration?[Xe] 6s2 4f14 5d9 Mercury Gold Platinum Thallium

Gold

What noble gas should be used to write the shorthand configuration for Te? Ar Kr Xe Sb

Kr

Which ionic bond is stronger MgCl2 SrCl2 BaCl2

MgCl2

Which element has a configuration of 1s2 2s2 2p6? Neon Helium Argon Krypton

Neon

The atom with the largest atomic radius in Group 18 is - Ar He Kr Rn

Rn

What is NOT A CAUSE for why electronegativity increases across the period in the periodic table? Shielding effect increases Number of protons increases Energy levels are closer to the nucleus Effective nuclear charge becomes greater

Shielding effect increases

Which element has electronic configuration of 1s2 2s2 2p6 3s2 3p2 C Si Mg Be

Si

Which of the following will have a larger radius than Zinc? Gallium Aluminum Magnesium Strontium

Strontium

The particle-level diagram above represents the structure of solid KFKF. Although the molar mass of KCl is greater than that of KF, the density of KCl is actually less than that of KF. Which of the following representations of the structure of KCl best helps to explain this phenomenon?

The diagram shows that the chloride ions (-) are larger than the fluoride ions, which causes the interionic distances in the solid to increase to the point where the effect of the larger spacing among ions in KClKCl is greater than the effect of the larger mass of the chlorine on the density. - photo w large (-) and small (+)

What atom matches this electron configuration? 1s2 2s2 2p6 3s2 3p6 4s2 3d10 Zinc Copper Nickel Germanium

Zinc

What atom matches this electron configuration?1s2 2s2 2p6 3s2 3p6 4s2 3d10 Zinc Copper Nickel Germanium

Zinc

What is the abbreeviate noble gas electron for Sulfur atom? [Ar] 3p4 [He] 3s23p4 [Ne] 3s23p4 [Na] 3s23p4

[Ne] 3s23p4

What is the shorthand electron configuration for Sulfur atom? [Ar] 3p4 [He] 3s23p4 [Ne] 3s23p4 [Na] 3s23p3

[Ne] 3s23p4

Which of the following is the correct abbreviated noble gas electron configuration for chlorine? [Ne]3s23p5 [He]2s22p63s23p5 [Mg]3p5 [Ne]1s22s22p63s23p5

[Ne]3s23p5

Each row on the periodic table represents: an energy level a sublevel an electron an orbital

an energy level

As electric charges get closer together, the force between them... becomes weaker becomes stronger stays the same disapears

becomes stronger

An element with an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 refers to _________. sulfur magnesium calcium krypton

calcium

What is a positively-charged ion which forms when an atom loses electrons? atom ion cation anion

cation

Which shells is NOT found in the 3rd energy level? s p d f

f

What does electronegativity do as you go across a period? decrease no pattern stay the same increase

increase

What is the amount of energy required to remove an electron from an atom? atomic energy ionization energy ionic energy electron energy

ionization energy

Francium (Fr) has the lowest ionization energy in Group 1 because - it has the smallest number of valence electrons it has the greatest atomic mass it has the greatest number of protons, so it attracts its electrons the strongest its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

What elements have zero electronegativity? metals nonmetals metalloids noble gases

noble gases

The 4 orbitals are s, p, d, f a, b, c, d 2, 4, 6, 8

s, p, d, f

There are 4 different types of subshells s,p,d,f true false

true