Chemistry- Chapter 4 and 6
s, p, d, f orbitals
1,3,5,7
Au is the symbol for A) gold. B) silver. C) argon. D) aluminum. E) sodium.
A)
sodium A) So B) Na C) No D) Sm E) Au
B)
Elements in group 2A(2) of the periodic table form ions with a charge of A) 1+. B) 1-. C) 2+. D) 3+. E) 0.
C)
Tin
Sn
Nickle
Symbol: Ni Atomic Number: 28
Zinc
Zn
In a chemical formula
•the symbols and subscripts are written in the lowest whole-number ratio of the atoms or ions. •the sum of ionic charges in the formula equals zero. •the total positive charge = total negative charge
To calculate atomic mass
•use the experimental percent abundance of each isotope of the element. •multiply the percent abundance by the atomic mass of that isotope. •sum the total mass of all isotopes.
Naturally occurring carbon consists of three isotopes: 12 C, 13 C, and 14 C. State the number of protons, neutrons, and electrons in each of the three isotopes.
12C6 6p, 6n, 6e 13C6 6p, 7n, 6e 14C6 6p, 8n, 6e
A polar covalent bond is found in which of these compounds? A) H2O B) F2 C) NaCl D) H2 E) N2
A)
A sample of silicon has three naturally occurring isotopes: Si-28 (mass 28.0 amu); Si-29 (mass 29.0 amu) and Si-30 (mass = 30.0 amu). If the average atomic mass of silicon is 28.1 amu, which isotope is the most abundant? A) Si-28 B) Si-29 C) Si-30 D) All isotopes have the same natural abundance.
A)
Ca is the symbol for A) calcium. B) carbon. C) cobalt. D) copper. E) cadmium.
A)
Consider a neutral atom with 30 protons and 34 neutrons. The atomic number of the element is A) 30. B) 32. C) 34. D) 64. E) 94.
A)
Consider a neutral atom with 30 protons and 34 neutrons. The number of electrons in this atom is A) 30. B) 32. C) 34. D) 64. E) 94.
A)
How many electrons will lithium gain or lose when it forms an ion? A) lose 1 B) gain 5 C) lose 2 D) lose 3 E) gain 1
A)
Identify the noble gas in the following list. A) helium B) nitrogen C) oxygen D) gold E) chlorine
A)
If the electronegativity difference between elements X and Y is 2.1, the bond between the elements XY is A) ionic. B) nonpolar ionic. C) nonpolar covalent. D) polar covalent. E) impossible.
A)
The Group 8A(18) elements A) are unreactive and are rarely found in combination with other elements. B) are good conductors of electricity. C) melt at high temperatures. D) are liquids at room temperature. E) react vigorously with water.
A)
The VSEPR theory allows us to determine the most favorable A) shape of a molecule. B) charge on an ion. C) color of a compound. D) bond type for a molecule. E) formula for a compound.
A)
The ability of an atom to attract the shared electrons in a covalent bond is its A) electronegativity. B) bonding ability. C) polarity. D) ionic character. E) nonpolarity.
A)
The ammonia molecule ( NH3) is A) a polar molecule with polar bonds. B) a nonpolar molecule with polar bonds. C) a nonpolar molecule with nonpolar bonds. D) a polar molecule with nonpolar bonds. E) a polar molecule with ionic bonds.
A)
The carbon tetrachloride molecule, CCl4 , has the shape of a A) tetrahedron. B) square. C) cube. D) circle. E) sphere.
A)
The correct formula for the compound formed from Mg and S is A) MgS. B) MgS2. C) Mg2S. D) Mg2S2 E) Mg2S3
A)
The correct symbol for the isotope of potassium with 22 neutrons is A) 41K19. B) 19K41. C) 37P15. D) 15P37. E) 22K19
A)
The shape of the carbon dioxide (CO2) is A) linear. B) square. C) pyramidal. D) hexagonal. E) bent.
A)
The strongest interactions in the compound sodium fluoride, NaF, are examples of A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces.
A)
Valence electrons are electrons located A) in the outermost energy level of an atom. B) in the nucleus of an atom. C) in the innermost energy level of an atom. D) throughout the atom. E) in the first three shells of an atom.
A)
What is the correct formula for the oxide ion? A) O2- B) O- D) O2+ E) O3+
A)
What is the electron configuration for aluminum? A) 1s 22s 22p 63s 23p 1 B) 1s 22s 22p 63s 23p 3 C) 1s 22s 22p 63s 23p 5 D) 1s 22s 22p 63s 23p 6 E) 1s 22s 22p 63s 23p 8
A)
What is the formula of a compound that contains Na+ and PO43- ions? A) Na3PO4 B) NaPO4 C) Na2PO3 D) Na3PO3 E) Na3P
A)
What is the formula of the nitride ion? A) N3- B) NO2- C) NO3 3- D) NO32- E) NO3-
A)
Which of the following descriptions of a subatomic particle is correct? A) A proton has a positive charge and a mass of approximately 1 amu. B) An electron has a negative charge and a mass of approximately 1 amu. C) A neutron has no charge and its mass is negligible. D) A proton has a positive charge and a negligible mass. E) A neutron has a positive charge and a mass of approximately 1 amu.
A)
Which of the following elements has the lowest electronegativity? A) Li B) C C) N D) O E) F
A)
Which of the following elements is a nonmetal? A) nitrogen B) sodium C) iron D) silver E) calcium
A)
Which of the following is NOT true for the atoms 13N, 14N, and 15N? A) They all have the same mass number. B) They are isotopes. C) They all have the same atomic number. D) They all have 7 protons. E) They all have 7 electrons.
A)
aluminum A) Al B) Am C) Au D) Sn E) Ag
A)
Using the periodic table, write the group number, the period, and the valence electron configuration for the following: A. calcium B. lead
A. Calcium is in Group 2A (2), Period 4. It has a valence electron configuration of 4s2. B. Lead is in Group 4A (14), Period 6. It has a valence electron configuration of 6s26p2
Complete each of the following statements with decreasesor increases. A. Going down Group 6A (16), the ionization energy _______. B. Going across Period 3, from left to right, the atomic size _______. C. Going down Group 2A (2), the metallic character _______
A. Going down Group 6A (16), the ionization energy decreases. B. Going across Period 3, from left to right, the atomic size decreases. C. Going down Group 2A (2), the metallic character increases
Write the atomic symbols for atoms with the following subatomic particles: A. 8 protons 8 neutrons 8 electrons B. 17 protons 20 neutrons 17 electrons C. 47 protons 60 neutrons 47 electrons
A. O B.Cl C.Ag
Write the names of the following compounds. A.CaO___________ B.Al2O3___________ C.MgCl2___________
A. The name of CaO is calcium oxide. B. The name of Al2O3 is aluminum oxide. C. The name of MgCl2 is magnesium chloride.
Write chemical formulas for the following compounds: A. nickel(II) sulfide B. zinc chloride C. iron(III) oxide
A.nickel(II) sulfideNiS B.zinc chlorideZnCl2 C.iron(III) oxideFe2O3
Select the correct formula for each of the following ionic compounds. 1.Na+ and O2− A.NaO B.Na2O C.NaO2 2.Al3+ and Cl− A.AlCl3 B.AlCl C.Al3Cl 3.Mg2+ and N3− A.MgN B.Mg2N3 C.Mg3N2
B A. C.
According to the Atomic Theory, A) all atoms are different. B) atoms are neither created nor destroyed during a chemical reaction. C) atoms of the same element combine to form compounds. D) all matter is made up of tiny particles called electrons. E) a compound can contain different numbers of atoms as long as it has the same kinds of atoms.
B)
Choose the best electron-dot structure for CH2Cl2
B)
Consider an isotope of sodium with a mass number of 25. The number of neutrons in this isotope of sodium is A) 11. B) 14. C) 16. D) 25. E) 32.
B)
Double and triple bonds form because A) the atoms involved have high electronegativities. B) single covalent bonds do not give all of the atoms in the molecule eight valence electrons. C) one of the atoms in the molecule has more than eight valence electrons. D) the ions involved have charges larger than one. E) there is at least one hydrogen atom involved in the bond.
B)
Given the following: X, X, X, and X. Which are isotopes of each other? A) X and X are isotopes of each other; and X and X are isotopes of each other. B) X and X are isotopes of each other. C) X, X, X, and X are isotopes of each other. D) None are isotopes of each other.
B)
How many electrons will chlorine gain or lose when it forms an ion? A) lose 1 B) gain 1 C) lose 7 D) gain 2 E) lose 3
B)
In an atom, the nucleus contains A) an equal number of protons and electrons. B) all the protons and neutrons. C) all the protons and electrons. D) only neutrons. E) only protons.
B)
In an electron-dot structure of an element, the dots are used to represent A) all of the electrons in the atom. B) the valence electrons. C) the electron arrangement. D) only the electrons that will participate in bond formation. E) the electrons that the element will gain when it forms a compound.
B)
Ionic bonding is expected in which of these compounds? A) Cl2 B) KF C) OF2 D) HF E) H2
B)
Ionization energy is A) the energy an ion acquires from an electron. B) the energy needed to remove the least tightly bound electron. C) highest for metals in Group 1A (1). D) higher for potassium than for lithium. E) None of the above.
B)
The atomic size of atoms A) increases going across a period. B) decreases going across a period. C) decreases going down within a group. D) does not change going across a period. E) None of the above.
B)
The bond in Cl2 is a(n) A) ionic bond. B) nonpolar covalent bond. C) metallic bond. D) polar ionic bond. E) no bond.
B)
The carbon tetrachloride molecule, CCl4 , is A) a polar molecule with polar bonds. B) a nonpolar molecule with polar bonds. C) a nonpolar molecule with nonpolar bonds. D) a polar molecule with nonpolar bonds. E) a polar molecule with ionic bonds.
B)
The elements sodium, magnesium, and silicon A) are isotopes of each other. B) are in the same period of elements. C) have the same number of neutrons. D) are in the same group. E) have the same mass number.
B)
The formula of copper(I) sulfide is A) CuS. B) Cu2S. C) Cu2(SO4)3 .D) CuSO4. E) CuS2.
B)
The ionization energy of atoms A) decreases going across a period. B) decreases going down within a group. C) increases going down within a group. D) does not change going down within a group. E) None of the above.
B)
The mass number of an atom can be calculated from A) the number of electrons. B) the number of protons plus neutrons. C) the number of protons. D) the number of electrons plus protons. E) the number of neutrons.
B)
The name of the Cu+ ion is A) copper(II). B) copper(I). C) cobalt. D) copper. E) cuprum.
B)
The name of the HSO4- ion is A) sulfate. B) hydrogen sulfate. C) sulfite. D) hydrogen sulfite. E) sulfide.
B)
The number of electrons in the outer energy level of a neutral atom of boron (atomic number 5) is A) 2. B) 3. C) 5. D) 8. E) 10.
B)
The strongest interactions between molecules of ammonia ( NH3) are A) ionic bonds. B) hydrogen bonds. C) polar covalent. D) dipole-dipole. E) dispersion forces.
B)
The water molecule has a dipole with the negative portion A) localized between the hydrogen atoms. B) pointing toward the oxygen atom. C) localized on one of the hydrogens. D) pointing from the oxygen through the hydrogen atoms. E) surrounding the molecule.
B)
What elements are in hydroxyapatite, Ca5 (PO4)3OH, a major compound in human bones and teeth? A) carbon, potassium, oxygen, hydrogen B) calcium, phosphorus, oxygen, hydrogen C) carbon, phosphorus, oxygen, helium D) calcium, phosphorus, oxygen, helium E) carbon, potassium, oxygen, helium
B)
What is the abbreviated electron configuration for nickel (atomic number 28)? A) [He]2s 22p 3 B) [Ar]4s 23d 8 C) [Kr]4s 23d 8 D) [Ar]4s 24p 4 E) [Ar]3d 8
B)
What is the correct formula for the iron(II) ion? A) Fe+ B) Fe2+ C) Fe3+ D) Fe2- E) Fe3-
B)
What is the element with the abbreviated electron configuration [Kr]5s24d8? A) Ni B) Pd C) Pt D) Kr E) Xe
B)
What is the element with the electron configuration 1s22s22p63s23p5? A) Be B) Cl C) F D) S E) Ar
B)
What is the formula of carbon tetraiodide? A) CI B) CI4 C) C4I D) CI3 E) C2I4
B)
Which element would have physical and chemical properties similar to chlorine? A) Ar B) Br C) S D) O E) P
B)
Which of the following compounds contains a polar covalent bond? A) NaF B) HCl C) Br2 D) MgO E) O2
B)
Which of the following electron configurations is impossible? A) 1s 22s 22p 63s 23p 1 B) 1s 22s 42p 63s 23p 3 C) 1s 22s 22p 63s 23p 5 D) 1s 22s 22p 63s 23p 6 E) 1s 22s 22p 63s 23p 3
B)
A group of covalently bonded atoms that has an overall electrical charge is called a(n) A) ionic compound. B) anion. C) polyatomic ion. D) cation. E) molecule.
C)
A(n) ________ is the smallest neutral unit of two or more atoms held together by a covalent bond. A) ionic compound B) nucleus C) molecule D) formula E) unit
C)
Fe2(SO4)3 is called A) iron sulfate. B) iron(II) sulfate. C) iron(III) sulfate. D) diiron trisulfate. E) iron trisulfate.
C)
How many lone pairs of electrons are in the electron-dot structure of H2O? A) 0 B) 1 C) 2 D) 3 E) 4
C)
How many valence electrons are in the electron-dot structures for the elements in group 3A(13)? A) 1 B) 2 C) 3 D) 4 E) 6
C)
Of the elements: B, C, F, Li, and Na, the element with the smallest atomic radius is A) B. B) C. C) F. D) Li. E) Na.
C)
Of the elements: B, C, F, Li, and Na. The element with the highest ionization energy is A) B. B) C. C) F. D) Li. E) Na.
C)
Of the elements: B, C, F, Li, and Na. The element with the least metallic character is A) B. B) C. C) F. D) Li. E) Na.
C)
Semiconductors are located in the periodic table on (or in) the A) left side of the table. B) right side of the table. C) line dividing metals from nonmetals in the table. D) first period of the table. E) last period of the table.
C)
The electron arrangement of any particular atom shows A) the number of isotopes possible. B) a description of the shape of each energy level. C) the number of electrons in each energy level. D) a diagram of an atomic nucleus. E) the maximum number of electrons each energy level can hold.
C)
The formula for a molecule formed from N and Cl would be A) NCl. B) NCl2 C) NCl3 D) N3Cl. E) NCl5
C)
The ion of aluminum is A) Al+. B) Al2+. C) Al3+. D) Al3- E) Al2-
C)
The name of PbO2 is A) lead dioxide. B) lead(II) oxide. C) lead(IV) oxide. D) plumbum oxide. E) lead oxygen.
C)
The number of electron levels in a magnesium atom is A) 1. B) 2. C) 3. D) 4. E) 5.
C)
The number of valence electrons found in an atom of a Group A element is equal to A) its atomic number. B) its mass number. C) its group number. D) eight. E) eight minus the group number.
C)
The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons.
C)
The shape of the ammonia molecule ( NH3) is A) linear. B) square. C) pyramidal. D) hexagonal. E) octagonal.
C)
What is the formula for aluminum nitrite? A) Al2NO2 B) AlNO3 C) Al(NO2)3 D) Al2(NO3)3 E) Al2(NO2)2
C)
What is the ionic charge of an ion with 13 protons and 10 electrons? A) 1+ B) 2+ C) 3+ D) 2- E) 3-
C)
What is the symbol of the element in Period 4 and Group 2? A) Be B) Mg C) Ca D) C E) Si
C)
Which of the following compounds contains an ionic bond? A) NH3 B) H2O C) CaO D) H2 E) CH4
C)
Which of the following gives the correct numbers of protons, neutrons, and electrons in a neutral atom of 118Sn50? A) 118 protons, 50 neutrons, 118 electrons B) 118 protons, 118 neutrons, 50 electrons C) 50 protons, 68 neutrons, 50 electrons D) 68 protons, 68 neutrons, 50 electrons E) 50 protons, 50 neutrons, 50 electrons
C)
Which of the following is a characteristic of the modern periodic table? A) A group is a horizontal row on the periodic table. B) A period is a column on the periodic table. C) The elements in each group have similar chemical properties. D) The B groups contain the representative elements. E) The A groups contain the transition elements.
C)
Which of the following is the correct electron-dot structure for carbon? A) B) C) D) E)
C)
Which one of the following compounds contains an ion with a 3+ charge? A) KCl B) Na2O C) FeCl3 D) CuCl E) MgCl2
C)
iron A) Ir B) Fs C) Fe D) In E) FE
C)
silver A) S B) Si C) Ag D) Au E) AG
C)
Exceptions to these rules are the following:
CN−cyanide OH−hydroxide
One letter element symbols
Carbon-C Nitrogen-N Fluorine-F Oxygen-O
Halogens form 4 polyatomic ions with oxygen. Each has a −1 charge
ClO4−perchlorate ClO3−chlorate ClO2−chlorite ClO−hypochlorite
Two letter element symbols
Cobalt-Co Ca-Calcium Al-Aluminum Mg-Magnesium
A Roman numeral equal to the ion charge is placed in parentheses immediately after the metal name
Cu2+copper(II) Pb2+lead(II) Cu+copper(I) Pb4+lead(IV) Fe2+iron(II) Cr2+chromium(II) Fe3+iron(III) Cr3+chromium(III)
A sample of chlorine has two naturally occurring isotopes. The isotope Cl-35 (mass 35.0 amu) makes up 75.8% of the sample, and the isotope Cl-37 (mass = 37.0 amu) makes up 24.3% of the sample. What is the average atomic mass for chlorine? A) 36.0 amu B) 35 amu C) 36.6 amu D) 35.5 amu E) 35.521 amu
D)
Consider a neutral atom with 30 protons and 34 neutrons. The mass number for this atom is A) 30. B) 32. C) 34. D) 64. E) 94.
D)
How many electrons will aluminum gain or lose when it forms an ion? A) lose 1 B) gain 5 C) lose 2 D) lose 3 E) gain 1
D)
How many valence electrons are in the electron-dot structure of H2O? A) 2 B) 4 C) 6 D) 8 E) 10
D)
Hydrogen sulfide, H2 S, has a shape similar to A) carbon dioxide. B) carbon monoxide. C) hydrogen chloride. D) water. E) carbon tetrachloride.
D)
In a molecule with covalent bonding A) oppositely charged ions are held together by strong electrical attractions. B) atoms of metals form bonds to atoms of nonmetals. C) atoms of different metals form bonds. D) atoms are held together by sharing electrons. E) atoms of noble gases are held together by attractions between oppositely charged ions.
D)
Isotopes are atoms of the same element that have A) different atomic numbers. B) the same atomic numbers but different numbers of protons. C) the same atomic numbers but different numbers of electrons. D) the same atomic number but different numbers of neutrons. E) the same atomic mass but different numbers of protons.
D)
The atomic mass of an element is equal to A) its mass number. B) its atomic number. C) one-twelfth of the mass of a carbon-12 atom. D) a weighted average mass of all of the naturally occurring isotopes of the element. E) the average mass of all of the naturally occurring isotopes of the element.
D)
The compound MgCl2 is named A) magnesium chlorine. B) magnesium dichloride. C) magnesium(II) chloride. D) magnesium chloride. E) dimagnesium chloride.
D)
The element in this list with chemical properties similar to magnesium is A) sodium. B) boron. C) carbon. D) strontium. E) chlorine.
D)
The elements lithium, sodium, and potassium A) are isotopes of each other. B) are in the same period of elements. C) have the same number of neutrons. D) are in the same group. E) have the same mass number.
D)
The maximum number of electrons that may occupy the third energy level is A) 2. B) 8. C) 10. D) 18. E) 32.
D)
The number of dots in the electron dot structure of carbon is A) one. B) two. C) three. D) four. E) five.
D)
The number of electrons in an ion with 20 protons and an ionic charge of 2+ is A) 24. B) 22. C) 20. D) 18. E) 16.
D)
The number of neutrons in an atom is equal to A) the atomic number. B) the mass number. C) the mass number + the atomic number. D) the mass number - the atomic number. E) the number of protons.
D)
The octet rule indicates that A) all of the noble gases have eight total electrons. B) all of the shells in an atom hold a maximum of 8 electrons. C) all of the Group A elements have 8 valence electrons. D) atoms lose, gain, or share valence electrons to have 8 valence electrons. E) the noble gases react with other compounds to get 8 valence electrons.
D)
The shape of the carbon tetrachloride molecule is A) linear. B) square. C) pyramidal. D) tetrahedral. E) octagonal.
D)
The shape of the water molecule ( H2O) is A) linear. B) tetrahedral. C) pyramidal. D) bent. E) octagonal.
D)
The smallest particle of an element that retains the characteristics of the element is a(n) A) electron. B) neutron. C) proton. D) atom. E) nucleus.
D)
The strongest interactions between molecules of hydrogen chloride are A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces.
D)
The types of compounds that use prefixes in their names are A) ionic compounds. B) ionic compounds involving transition metals. C) polyatomic ions. D) covalent compounds. E) compounds that contain polyatomic ions.
D)
To form an ion, a sodium atom A) gains one electron. B) gains two electrons. C) loses seven electrons. D) loses one electron. E) loses two electrons.
D)
What is the correct electron configuration for the lithium atom? A) 1s 3 B) 2s 1 C) 1s 12s 2 D) 1s 2 2s 1 E) 1s 22s 5
D)
What is the electron configuration for potassium (atomic number 19)? A) 1s 22s 22p 63s 23p 7 B) 1s 22s 22p 6 3s 23p 53d 2 C) 1s 22s 22p 83s 23p 5 D) 1s 22s 22p 63s 23p 64s 1 E) 1s 22s 22p 63s 23p 54s 1
D)
What is the mass number of an atom of potassium that has 20 neutrons? A) 15 B) 19 C) 35 D) 39 E) 59
D)
What is the symbol of the element in Group 4A(14) and Period 2? A) Be B) Mg C) Ca D) C E) Si
D)
Which of the following elements is a metal? A) nitrogen B) fluorine C) argon D) strontium E) phosphorus
D)
Which of the following elements is a noble gas? A) oxygen B) chlorine C) bromine D) argon E) nitrogen
D)
Which of the following is a characteristic of nonmetals? A) shiny B) malleable C) good conductors of heat D) low melting points E) good conductors of electricity
D)
Which of the following polyatomic ions has a 3- ionic charge? A) hydroxide B) nitrate C) sulfate D) phosphate E) bicarbonate
D)
Which of the following polyatomic ions has a positive charge? A) hydroxide B) sulfate C) hydrogen carbonate D) ammonium E) nitrate
D)
Which of the following properties is NOT a characteristic of the Group 1A(1) elements (alkali metals)? A) They are shiny. B) They are good conductors of heat. C) They react vigorously with water. D) Most of them are liquids at room temperature. E) They are good conductors of electricity.
D)
potassium A) P B) Po C) Pt D) K E) Ko
D)
An anion always A) has a positive charge. B) contains a group of two or more atoms with a positive charge. C) contains a metal and a nonmetal. D) forms covalent bonds. E) has a negative charge.
E)
An ionic compound A) has a net positive charge. B) has a net negative charge. C) contains only cations. D) contains only anions. E) has a net charge of zero.
E)
Choose the best electron-dot structure for OCl2
E)
How many electrons will iodine gain or lose when it forms an ion? A) lose 1 B) gain 5 C) lose 2 D) lose 3 E) gain 1
E)
How many valence electrons are in the electron-dot structure of CCl4 ? A) 0 B) 82 C) 6 D) 8 E) 32
E)
How many valence electrons does nitrogen have? A) one B) two C) three D) four E) five
E)
Identify the metalloid in the following list. A) sulfur B) fluorine C) silver D) copper E) germanium
E)
In a covalently bonded molecule, the number of electrons that an atom shares with others is usually equal to the number of electrons A) in the atom. B) in its nucleus. C) in all the atoms. D) in its ion. E) needed to give it a stable electron configuration.
E)
In ionic compounds, ________ lose their valence electrons to form positively charged ________. (5,2) A) metals; anions B) nonmetals; cations C) metals; polyatomic ions D) nonmetals; anions E) metals; cations
E)
Of the elements: B, C, F, Li, and Na. The element with the most metallic character is A) B. B) C. C) F. D) Li. E) Na
E)
Of the elements: B, C, F, Li, and Na. The element with the smallest ionization energy is A) B. B) C. C) F. D) Li. E) Na.
E)
Of the elements: B, C, F, Li, and Na., the element with the largest atomic radius is A) B. B) C. C) F. D) Li. E) Na.
E)
The atomic number of an atom is equal to the number of A) nuclei. B) neutrons. C) neutrons plus protons. D) electrons plus protons. E) protons.
E)
The correct formula for a compound formed from the elements Al and O is A) AlO. B) Al2O. C) Al3O2 . D) AlO3 . E) Al2O3 .
E)
The correct name for the compound N2O3 is A) nitrogen oxide. B) nitrogen trioxide. C) dinitride trioxide. D) dinitrogen oxide. E) dinitrogen trioxide.
E)
The correct name of the compound is NCl3 A) nitrogen chloride. B) trinitrogen chloride. C) nitrogen(III) chloride. D) nickel chloride. E) nitrogen trichloride.
E)
The number of dots in the electron dot structure of nitrogen is A) one. B) two. C) three. D) four. E) five.
E)
The strongest interactions between atoms of helium He are examples of A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces.
E)
The strongest interactions between molecules of hydrogen ( H2) are A) ionic bonds. B) hydrogen bonds. C) polar covalent. D) dipole-dipole. E) dispersion forces.
E)
The strongest interactions between molecules of iodine I2 are examples of A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces.
E)
What element has the electron configuration 1s22s22p63s23p2? A) carbon B) oxygen C) sulfur D) iron E) silicon
E)
What is the correct formula for iron(III) sulfide? A) Fe2S2 B) Fe2S C) FeS D) FeS2 E) Fe2S3
E)
What is the symbol for the ion with 19 protons and 18 electrons? A) F+ B) F C) Ar+ D) K- E) K+
E)
Which of the following elements does NOT exist as a diatomic molecule? A) hydrogen B) nitrogen C) chlorine D) oxygen E) carbon
E)
Which of the following substances contains a nonpolar covalent bond? A) H2O B) NaCl C) NH3 D) MgF2 E) N2
E)
Which one of the following elements forms two or more ions with different ionic charges? A) K B) F C) Ca D) O E) Fe
E)
he name of Al2(SO4)3 is A) aluminum(III) sulfate. B) dialuminum trisulfate. C) dialuminum sulfate. D) dialuminum trisulfide. E) aluminum sulfate.
E)
Elements
Elements •are pure substances from which all other things are built. •cannot be broken down into simpler substances.
Given the elements C, N, and F, A. which is the largest atom? B. which has the highest ionization energy? C. which belongs to Group 5A (15)?
Given the elements C, N, and F, A. which is the largest atom? C B. which has the highest ionization energy? F C. which belongs to Group 5A (15)? N
groups 3A through 6A (13-16)
No common names
Given the atomic symbols, determine the number of protons, neutrons, and electrons 16O8
Protons= 8 Neutrons=8 Mass= 16-protons= 8 neutrons
When a related ion has one less oxygen, its name ends in ite.
SO32−sulfite PO33−phosphite NO2−nitrite
Names of most common polyatomic ions end in ate
SO42−sulfate PO43−phosphate NO3−nitrate
Lithium consists of two naturally occurring isotopes, 6 Li and 7 Li. Use the periodic table to predict which isotope is the more prevalent one. (According to the periodic table, the atomic mass of lithium is 6.941 amu.)
Since the total atomic mass of 7 Li is closer to 7, the mass number of 7 Li, the more prevalent isotope is 7 Li
Atomic Spectrum
When light from a heated element passes through a prism, it separates into distinct lines of color separated by dark areas called an atomic spectrum. Each element has its own unique atomic spectrum
periods
are horizontal rows of elements, counted from top to bottom of the table as Periods 1−7
Number of protons =
atomic number
Atomic size •is determined by the atom's
atomic radius,the distance between the nucleus and the outermost electrons. •increases for representative elements from top to bottom of the periodic table. •decreases within a period as a result of increased number of protons in the nucleus
Lewis symbols represent the valence electrons as
dots placed on sides of the symbol for an element
An element with metallic character is one that loses valence electrons
easily
Ionization energy decreases down a
group and increases going across a period from left to right
Metallic character
is more prevalent in metals on the left side of the periodic table. •is less for nonmetals on the right side of the periodic table that do not lose electrons easily. •decreases going down a group, as electrons are farther away from the nucleus.
Covalent bonds occur when nonmetal atoms share electrons to attain a
noble gas arrangement
Ionic bonds occur when valence electrons of a metal atom are transferred to the atom of a
nonmetal.
Valence electrons are the electrons in the
outermost energy level. •The group number gives the number of valence electrons for the representative elements
ionic compounds consist of
positive and negative charges held together by the strong electrical attractions between oppositely charged ions
The group number gives the number of valence electrons for the
representative elements
For neutral atoms, the net charge is
zero. number of protons = number of electrons -Atoms Are Neutral For neutral atoms, the net charge is zero. number of protons = number of electrons Aluminum has 13 protons and 13 electrons. The net (overall) charge is zero. 13 protons (13+) + 13 electrons (13) = 0
Metalloids are located along the heavy
zigzag line
Ionization energy is the energy required to remove one of the outermost electrons
•As the distance from the nucleus to the valence electrons increases, the ionization energy decreases. •The ionization energy is low for metals and high for the nonmetals.
Write the formula and symbol of an ion with 16 protons and 18 electrons
•The element with 16 protons is sulfur, with the symbol S. •An ion of sulfur with 18 electrons gives sulfur a charge of 2−. •The sulfide ion is S2−
Polyatomic ions
•are a group of covalently bonded atoms with an overall ionic charge. •often consist of a nonmetal such as phosphorus, sulfur, carbon, or nitrogen covalently bonded to oxygen atoms .•usually have a 1−, 2−, or 3− charge. •have a negative charge, except for NH4+, ammonium, which has a positive charge
Ionic compounds
•consist of positive and negative ions. •have attractions called ionic bonds between positively and negatively charged ions. •have high melting points. •are solids at room temperature.
When naming an ionic compound
•the name of the metal is written first and is the same as the name of the element. •the name of the nonmetal is the first syllable of the nonmetal name + ide ending and is written second. •a space is placed between the name of the metal and nonmetal ion.
Nonmetals located on the right side of the periodic table are
-are dull, brittle, and poor conductors but often good insulators. -have low densities and melting points
List all of the elements that match the description. A.metals in Group 4A (14) Sn, Pb, C, Si, Ge B.nonmetals in Group 5A (15) Bi, N, P, As, Sb C.metalloids in Group 4A (14) C, Si, Ge, Sn, Pb
List all of the elements that match the description. A. metals in Group 4A (14) Sn, Pb B. nonmetals in Group 5A (15) N, P C. metalloids in Group 4A (14) Si, Ge
Gold
Symbol: Au Atomic Mass: 197.0 Atomic Number: 79
Boron
Symbol: B Atomic Mass: 10.81 Atomic Number: 5
Barium
Symbol: Ba Atomic Mass: 137.3 Atomic Number: 56
Bromine
Symbol: Br Atomic Mass: 79.90 Atomic Number: 35
carbon
Symbol: C Atomic Mass: 12.01 Atomic Number: 6
Calcium
Symbol: Ca Atomic Mass: 40.08 Atomic Number: 20
Lead
Symbol: Pb Atomic Mass: 207.2 Atomic Number: 82
Titanium
Symbol: Ti Atomic Mass: 47.87 Atomic Number: 22 -Titians
Group 1A elements (1)
alkali metals
electrons
have a negative (-) charge
protons
have a positive (+) charge
Neutrons
have no charge
Metals are located to the
left
Which of the following subatomic particles fits each of the descriptions below? protons, neutrons, or electrons A. found outside the nucleus B. have a positive charge C.have mass but no charge
A. Electron B. Proton C.Neutron
Give the names of the elements with the following symbols: A. P B. Al C. Mn D. H E. K
A. P-Phosphorus B. Al-Aluminum C. Mn-Manganese D. H-Hydrogen E. K-Potassium
Write the correct chemical symbols for each of the following elements: A. iodine B. iron C. magnesium D. zinc E.nitrogen
A. iodine- I B. iron-Fe C. magnesium-Mg D. zinc-Zn E.nitrogen-N
An atom of lead (Pb) has a mass number of 207. A. How many protons are in the nucleus? B. How many neutrons are in the nucleus? C. How many electrons are in the atom?
A.82 B.125 C.82
Identify each of the following elements as a metal, a nonmetal, or a metalloid: A.sodium B.chlorine C.silicon D.iron E.carbon
A.sodium -metal B.chlorine-non-metal C.silicon -mellatoid D.iron-metal E.carbon-non metal
Chemical symbols from Latin words
Ag silver (argentum) Au gold (aurum)
groups 7A (17)
Halogens
Uranium-
Symbol- U Number-235 an unstable, fissionable isotope of uranium -Uranus
Silver
Symbol: Ag Atomic Mass: 107.9 Atomic Number: 47
Aluminum
Symbol: Al Atomic Mass: 26.98 Atomic Number: 13
Argon
Symbol: Ar Atomic Mass: 39.95 Atomic Number: 18
Arsenic
Symbol: As Atomic Mass: 74.92 Atomic Number: 33
Iodine(2)
Symbol: I Atomic Mass: 126.9 Atomic Number: 53
Iodine
Symbol: I Atomic Mass: 126.9 Atomic Number: 53 ioedies- Violet
Potassium
Symbol: K Atomic Mass: 39.10 Atomic Number: 19
Platinum
Symbol: Pt Atomic Mass: 195.1 Atomic Number: 78
Radium
Symbol: Ra Atomic Mass: Atomic Number: 88
Sulfur
Symbol: S Atomic Mass: 32.07 Atomic Number: 16
Silicon
Symbol: Si Atomic Mass: 28.09 Atomic Number: 14
Group numbers are written where ?
at the top of each vertical column. •Use the letter A for representative elements (Groups 1A-8A). •Use the letter B for transition elements (Groups 3B-12B)
unlike charges
attract one another
Groups 8A (18)
noble gases
In the periodic table, elements are arranged according to
properties
Atomic number = number of protons—for example,
•the atomic number of H is 1; every H atom has one proton. •the atomic number of C is 6; every C atom has six protons. •the atomic number of Cu is 29; every Cu atom has 29 protons.
Macrominerals —Ca, P, K, Cl, S, Na, and Mg— located in Period 3 and Period 4—are involved in
•the formation of bones and teeth. •maintenance of heart and blood vessels, musclecontraction, nerve impulses, and acid-base balance of body fluids. •regulation of cellular metabolism
Identify the element described by each of the following groups and periods: Group 7A (17), Period 4 A. Br B. Cl C. Mn Group 2A (2), Period 3 A. berylliumB. boron C. magnesium Group 5A (15), Period 2 A. phosphorus B. arsenicC. nitrogen
1.A 2.C 3.C
Cadmium
Symbol: Cd Atomic Mass: 112.4 Atomic Number: 48
chlorine
Symbol: Cl Atomic Mass: 35.45 Atomic Number: 17
Chlorine
Symbol: Cl Atomic Mass: 35.45 Atomic Number: 17 -Choloros-Yellow-green
Curium
Symbol: Cm Atomic Mass: Atomic Number: 96 -Marie and Pierre curie
Copernicium
Symbol: Cn Atomic Mass: Atomic Number: 112 -nicolus copernicus
cobalt
Symbol: Co Atomic Mass: 58.93 Atomic Number: 27co
copper
Symbol: Cu Atomic Mass: 63.55 Atomic Number: 29
Fluorine
Symbol: F Atomic Mass: 19.00 Atomic Number: 9
Iron
Symbol: Fe Atomic Mass: 55.85 Atomic Number: 26
Gallium
Symbol: Ga Atomic Mass: 69.72 Atomic Number: 31
Hydrogen
Symbol: H Atomic Mass: 1.01 Atomic Number: 1
Helium
Symbol: He Atomic Mass: 4.00 Atomic Number: 2
Mercury
Symbol: Hg Atomic Mass: 200.6 Atomic Number: 80
Lithium
Symbol: Li Atomic Mass: 3 Atomic Number: 6.94
Magnesium (2)
Symbol: Mg Atomic Mass: 24.31 Atomic Number: 12
Magnesium
Symbol: Mg Atomic Mass: 24.31 Atomic Number: 12 -Magnesia, a mineral
Nitrogen
Symbol: N Atomic Mass: 14.01 Atomic Number: 7
Sodium
Symbol: Na Atomic Mass: 22.99 Atomic Number: 11
Neon
Symbol: Ne Atomic Mass: 20.18 Atomic Number: 10
Oxygen
Symbol: O Atomic Mass: 16.00 Atomic Number: 8
Phophorus
Symbol: P
Tennessine
Symbol: Ts Atomic Mass: Atomic Number: 117 -Tennesse
Group 2A (2) elements are called
alkaline earth metals
groups
contain elements with similar properties in vertical columns
An atom is the smallest particle of an
element that retains the characteristics of that element
Chemical symbol represents the names of the
elements. •consist of one to two letters and start with a capital letter.
Number of protons + neutrons =
mass number
Number of neutrons=
mass number - atomic number Note: Mass numbers are given for specific isotopes only
All atoms of an element have the same number of
protons and the same atomic number
Like charges
repel each other
mass of atom
sum of protons and neutrons
Nonmetals are located to
the right
Groups 3B-2B (3-12)
transition metals
Chemistry Link to Health: Elements Essential to Health Of all the elements,
•20 are essential for the well-being and survival of the human body. •four—oxygen, carbon, hydrogen, and nitrogen—make up 96% of our body mass. •most of our hydrogen and oxygen is found as water, which makes up 55 to 60% of our body mass
An atom consists of
•a nucleus, located in the center of the atom, that contains protons and neutrons and represents most of the mass of an atom. •electrons that occupy a large, empty space around the nucleus
Isotopes are
•are atoms of the same element. •have different mass numbers. •have the same number of protons but different numbers of neutrons. •can be distinguished by their atomic symbols
Metals, except for hydrogen located on the left of the periodic table, are :
•are shiny and ductile, and conduct heat and electricity. •are solids, except for mercury (Hg), which is a liquid.
In Dalton 's atomic theory , atoms are
•are tiny particles of matter. •of an element are similar to each other and different from those of other elements .•of two or more different elements combine to form compounds. •are rearranged to form new combinations in a chemical reaction. -Atoms are never created or destroyed during a chemical reaction
Group 2A (2) elements,the alkaline earth metals, are shiny but not as reactive as Group 1A metals. They include the following:
•beryllium (Be) •magnesium (Mg) •calcium (Ca) •strontium (Sr) •barium (Ba) •radium (Ra)
Metalloids located along the heavy zigzag line on the periodic table (except for aluminum and oganesson)
•exhibit properties of metals and nonmetals. •are better conductors than nonmetals but not as good as metals. •are used as semiconductors and insulators, because they can be modified to function as conductors or insulators
Group 7A (17)the halogens, are highly reactive and form compounds with most of the elements. Group 7A includes the following:
•fluorine (F) •chlorine (Cl) •bromine (Br) •iodine (I)
The atomic number
•is a whole number specific for each element. •is the same for all atoms of an element .•is equal to the number of protons in an atom .•appears above the symbol of an element in the periodic table.
Group 1A (1) the alkali metals, includes the following:
•lithium (Li) •sodium (Na) •potassium (K) •rubidium (Rb) •cesium (Cs)
The mass number
•represents the number of particles in the nucleus .•is equal to the number of protons + the number of neutrons. •is always a whole number. •the mass of a single atom does not appear in the periodic table.
