To what group number does each element belong (a) oxygen (b) aluminum (c) silicon (d)

What did Democritus contribute to our modern understanding of matter?

What are three main ideas in Daltons atomic theory?

Describe Rutherfords gold foil experiment and the results of that experiment. How did these results contradict the plum pudding model of the atom?

What are the main ideas in the nuclear theory of the atom?

List the three subatomic particles and their properties.

What is electrical charge?

Is matter usually charge-neutral? How would matter be different if it were not charge-neutral?

What does the atomic number of an element specify?

What is a chemical symbol?

List some examples of how elements got their names.

What was Dmitri Mendeleevs main contribution to our modern understanding of chemistry?

What is the main idea in the periodic law?

How is the periodic table organized?

What are the properties of metals? Where are metals found on the periodic table?

What are the properties of nonmetals? Where are nonmetals found on the periodic table?

Where on the periodic table are metalloids found?

What is a family or group of elements?

Locate each group of elements on the periodic table and list its group number. (a) alkali metals (b) alkaline earth metals (c) halogens (d) noble gases

What is an ion?

What is an anion? What is a cation?

Locate each group on the periodic table and list the charge of the ions it tends to form. (a) Group 1A (b) Group 2A (c) Group 3A (d) Group 6A (e) Group 7A

What are isotopes?

What is the percent natural abundance of isotopes?

What is the mass number of an isotope?

What notations are commonly used to specify isotopes? What do each of the numbers in these symbols mean?

What is the atomic mass of an element?

Which statements are inconsistent with Daltons atomic theory as it was originally stated? Why? (a) All carbon atoms are identical. (b) Helium atoms can be split into two hydrogen atoms. (c) An oxygen atom combines with 1.5 hydrogen atoms to form water molecules. (d) Two oxygen atoms combine with a carbon atom to form carbon dioxide molecules.

Which statements are consistent with Daltons atomic theory as it was originally stated? Why? (a) Calcium and titanium atoms have the same mass. (b) Neon and argon atoms are the same. (c) All cobalt atoms are identical. (d) Sodium and chlorine atoms combine in a 1:1 ratio to form sodium chloride.

Which statements are inconsistent with Rutherfords nuclear theory as it was originally stated? Why? (a) Helium atoms have two protons in the nucleus and two electrons outside the nucleus. (b) Most of the volume of hydrogen atoms is due to the nucleus. (c) Aluminum atoms have 13 protons in the nucleus and 22 electrons outside the nucleus. (d) The majority of the mass of nitrogen atoms is due to their 7 electrons.

Which statements are consistent with Rutherfords nuclear theory as it was originally stated? Why? (a) Atomic nuclei are small compared to the size of atoms. (b) The volume of an atom is mostly empty space. (c) Neutral potassium atoms contain more protons than electrons. (d) Neutral potassium atoms contain more neutrons than protons.

If atoms are mostly empty space, and atoms compose all ordinary matter, then why does solid matter seem to have no space within it?

Rutherfords experiment suggested that matter was not as uniform as it appears. What part of his experimental results implied this idea? Explain.

Which statements about electrons are true? (a) Electrons repel each other. (b) Electrons are attracted to protons. (c) Some electrons have a charge of and some have no charge. (d) Electrons are much lighter than neutrons.

Which statements about electrons are false? (a) Most atoms have more electrons than protons. (b) Electrons have a charge of . (c) If an atom has an equal number of protons and electrons, it will be charge-neutral. (d) Electrons experience an attraction to protons.

Which statements about protons are true? (a) Protons have twice the mass of neutrons. (b) Protons have the same magnitude of charge as electrons but are opposite in sign. (c) Most atoms have more protons than electrons. (d) Protons have a charge of .

Which statements about protons are false? (a) Protons have about the same mass as neutrons. (b) Protons have about the same mass as electrons. (c) Some atoms dont have any protons. (d) Protons have the same magnitude of charge as neutrons, but are opposite in sign.

How many electrons would it take to equal the mass of a proton?

A helium nucleus has two protons and two neutrons. How many electrons would it take to equal the mass of a helium nucleus?

What mass of electrons would be required to just neutralize the charge of 1.0 g of protons?

What mass of protons would be required to just neutralize the charge of 1.0 g of electrons?

Find the atomic number (Z) for each element. (a) Fr (b) Kr (c) Pa (d) Ge (e) Al

Find the atomic number (Z) for each element. (a) Si (b) W (c) Ni (d) Rn (e) Sr

How many protons are in the nucleus of an atom of each element? (a) Ar (b) Sn (c) Xe (d) O (e) Tl

How many protons are in the nucleus of an atom of each element? (a) Ti (b) Li (c) U (d) Br (e) F

List the symbol and atomic number corresponding to each element. (a) carbon (b) nitrogen (c) sodium (d) potassium (e) copper

List the symbol and atomic number corresponding to each element. (a) boron (b) neon (c) silver (d) mercury (e) curium

List the name and the atomic number corresponding to the symbol for each element. (a) Mn (b) Ag (c) Au (d) Pb (e) S

List the name and the atomic number corresponding to the symbol for each element. (a) Y (b) N (c) Ne (d) K (e) Mo

Fill in the blanks to complete the table.

Fill in the blanks to complete the table.

Classify each element as a metal, nonmetal, or metalloid. (a) Sr (b) Mg (c) F (d) N (e) As

Classify each element as a metal, nonmetal, or metalloid. (a) Na (b) Ge (c) Si (d) Br (e) Ag

Which elements would you expect to lose electrons in chemical changes? (a) potassium (b) sulfur (c) fluorine (d) barium (e) copper

Which elements would you expect to gain electrons in chemical changes? (a) nitrogen (b) iodine (c) tungsten (d) strontium (e) gold

Which elements are main-group elements? (a) Te (b) K (c) V (d) Re (e) Ag

Which elements are not main-group elements? (a) Al (b) Br (c) Mo (d) Cs (e) Pb

Which elements are alkaline earth metals? (a) sodium (b) aluminum (c) calcium (d) barium (e) lithium

Which elements are alkaline earth metals? (a) rubidium (b) tungsten (c) magnesium (d) cesium (e) beryllium

Which elements are alkali metals? (a) barium (b) sodium (c) gold (d) tin (e) rubidium

Which elements are alkali metals? (a) scandium (b) iron (c) potassium (d) lithium (e) cobalt

Classify each element as a halogen, a noble gas, or neither. (a) Cl (b) Kr (c) F (d) Ga (e) He

Classify each element as a halogen, a noble gas, or neither. (a) Ne (b) Br (c) S (d) Xe (e) I

To what group number does each element belong? (a) oxygen (b) aluminum (c) silicon (d) tin (e) phosphorus

To what group number does each element belong? (a) germanium (b) nitrogen (c) sulfur (d) carbon (e) boron

Which element do you expect to be most like sulfur? Why? (a) nitrogen (b) oxygen (c) fluorine (d) lithium (e) potassium

Which element do you expect to be most like magnesium? Why? (a) potassium (b) silver (c) bromine (d) calcium (e) lead

Which pair of elements do you expect to be most similar? Why? (a) Si and P (b) Cl and F (c) Na and Mg (d) Mo and Sn (e) N and Ni

Which pair of elements do you expect to be most similar? Why? (a) Ti and Ga (b) N and O (c) Li and Na (d) Ar and Br (e) Ge and Ga

Fill in the blanks to complete the table.

Fill in the blanks to complete the table.

Complete each ionization equation. (a) ____ (b) ____ (c) ____ (d) Cl + e ____ - CaCa2+ + O + 2e- NaNa+ +

Complete each ionization equation. (a) (b) ____ (c) ____ (d) Al + 3eI + e- Ba Ba2+ + Mg + 2e

Determine the charge of each ion. (a) oxygen ion with 10 electrons (b) aluminum ion with 10 electrons (c) titanium ion with 18 electrons (d) iodine ion with 54 electrons

Determine the charge of each ion. (a) tungsten ion with 68 electrons (b) tellurium ion with 54 electrons (c) nitrogen ion with 10 electrons (d) barium ion with 54 electrons

Determine the number of protons and electrons in each ion. (a) (b) (c) (d) Co3+ O2+ Ba2+ Na

Determine the number of protons and electrons in each ion. (a) (b) (c) (d) Ag+

Determine whether each statement is true or false. If false, correct it. (a) The ion contains 22 protons and 24 electrons. (b) The ion contains 53 protons and 54 electrons. (c) The ion contains 14 protons and 12 electrons. (d) The ion contains 8 protons and 10 electrons.

Determine whether each statement is true or false. If false, correct it. (a) The ion contains 29 protons and 26 electrons. (b) The ion contains 55 protons and 56 electrons. (c) The ion contains 32 protons and 34 electrons. (d) The ion contains 3 protons and 2 electrons.

Predict the ion formed by each element: (a) Rb (b) K (c) Al (d) O

Predict the ion formed by each element: (a) F (b) N (c) Mg (d) Na

Predict how many electrons will most likely be gained or lost by each element: (a) Ga (b) Li (c) Br (d) S

Predict how many electrons will most likely be gained or lost by each element: (a) I (b) Ba (c) Cs (d) Se

Fill in the blanks to complete the table.

Fill in the blanks to complete the table.

What are the atomic number and mass number for each isotope? (a) the hydrogen isotope with 2 neutrons (b) the chromium isotope with 28 neutrons (c) the calcium isotope with 22 neutrons (d) the tantalum isotope with 109 neutrons

How many neutrons are in an atom with each set of atomic numbers and mass numbers? (a) Z = 28, A = 59 (b) Z = 92, A = 235 (c) Z = 21, A = 46 (d) Z = 18, A = 42

Write isotopic symbols of the form for each isotope. (a) the oxygen isotope with 8 neutrons (b) the fluorine isotope with 10 neutrons (c) the sodium isotope with 12 neutrons (d) the aluminum isotope with 14 neutrons

Write isotopic symbols of the form X-A (for example, C-13) for each isotope. (a) the iodine isotope with 74 neutrons (b) the phosphorus isotope with 16 neutrons (c) the uranium isotope with 234 neutrons (d) the argon isotope with 22 neutrons

Write the symbol for each isotope in the form . (a) cobalt-60 (b) neon-22 (c) iodine-131 (d) plutonium-244

Write the symbol for each isotope in the form . (a) U-235 (b) V-52 (c) P-32 (d) Xe-144

Determine the number of protons and neutrons in each isotope: (a) (b) (c) (d) 7 14N 82 208Pb 28 266Ra 11 23Na

Determine the number of protons and neutrons in each isotope: (a) (b) (c) (d) 43 99Tc 86 222Rn 19 40K 15 33P

Carbon-14, present within living organisms and substances derived from living organisms, is often used to establish the age of fossils and artifacts. Determine the number of protons and neutrons in a carbon-14 isotope and write its symbol in the form Z AX.

Plutonium-239 is used in nuclear bombs. Determine the number of protons and neutrons in plutonium239 and write its symbol in the form Z AX.

Rubidium has two naturally occurring isotopes: Rb-85 with mass 84.9118 amu and a natural abundance of 72.17%, and Rb-87 with mass 86.9092 amu and a natural abundance of 27.83%. Calculate the atomic mass of rubidium.

Silicon has three naturally occurring isotopes: Si-28 with mass 27.9769 amu and a natural abundance of 92.21%, Si-29 with mass 28.9765 amu and a natural abundance of 4.69%, and Si-30 with mass 29.9737 amu and a natural abundance of 3.10%. Calculate the atomic mass of silicon.

Bromine has two naturally occurring isotopes (Br-79 and Br-81) and an atomic mass of 79.904 amu. (a) If the natural abundance of Br-79 is 50.69%, what is the natural abundance of Br-81? (b) If the mass of Br-81 is 80.9163 amu, what is the mass of Br-79?

Silver has two naturally occurring isotopes (Ag-107 and Ag-109). (a) Use the periodic table to find the atomic mass of silver. (b) If the natural abundance of Ag-107 is 51.84%, what is the natural abundance of Ag-109? (c) If the mass of Ag-107 is 106.905 amu, what is the mass of Ag-109?

An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu and a relative abundance of 57.4%, and isotope 2 has a mass of 122.9042 amu and a relative abundance of 42.6%. Find the atomic mass of this element and, referring to the periodic table, identify it.

Copper has two naturally occurring isotopes. Cu-63 has a mass of 62.939 amu and relative abundance of 69.17%. Use the atomic weight of copper to determine the mass of the other copper isotope.

Electrical charge is sometimes reported in coulombs (C). On this scale, 1 electron has a charge of Suppose your body acquires (millicoulombs) of charge on a dry day. How many excess electrons has it acquired? (Hint: Use the charge of an electron in coulombs as a conversion factor between charge and electrons.)

How many excess protons are in a positively charged object with a charge of (millicoulombs)? The charge of 1 proton is +1.6 * 10-19 C.

The hydrogen atom contains 1 proton and 1 electron. The radius of the proton is approximately 1.0 fm (femtometers), and the radius of the hydrogen atom is approximately 53 pm (picometers). Calculate the volume of the nucleus and the volume of the atom for hydrogen. What percentage of the hydrogen atoms volume is occupied by the nucleus?

Carbon-12 contains 6 protons and 6 neutrons. The radius of the nucleus is approximately 2.7 fm, and the radius of the atom is approximately 70 pm. Calculate the volume of the nucleus and the volume of the atom. What percentage of the carbon atoms volume is occupied by the nucleus?

Prepare a table such as Table 4.2 for the four different isotopes of Sr that have the following natural abundances and masses.

Determine the number of protons and neutrons in each isotope of chromium and use the following natural abundances and masses to calculate its atomic mass.

Fill in the blanks to complete the table.

Fill in the blanks to complete the table.

Europium has two naturally occurring isotopes: Eu151 with a mass of 150.9198 amu and a natural abundance of 47.8%, and Eu-153. Use the atomic mass of europium to find the mass and natural abundance of Eu-153.

Rhenium has two naturally occurring isotopes: Re-185 with a natural abundance of 37.40%, and Re-187 with a natural abundance of 62.60%. The sum of the masses of the two isotopes is 371.9087 amu. Find the masses of the individual isotopes.

Chapter 1 describes the difference between observations, laws, and theories. Provide two examples of theories from this chapter and explain why they are theories.

Chapter 1 describes the difference between observations, laws, and theories. Provide one example of a law from this chapter and explain why it is a law.

The atomic mass of fluorine is 19.00 amu, and all fluorine atoms in a naturally occurring sample of fluorine have this mass. The atomic mass of chlorine is 35.45 amu, but no chlorine atoms in a naturally occurring sample of chlorine have this mass. Explain the difference.

The atomic mass of germanium is 72.61 amu. Is it likely that any individual germanium atoms have a mass of 72.61 amu?

Copper has only two naturally occurring isotopes, Cu-63 and Cu-65. The mass of Cu-63 is 62.9396 amu, and the mass of Cu-65 is 64.9278 amu. Use the atomic mass of copper to determine the relative abundance of each isotope in a naturally occurring sample.

Gallium has only two naturally occurring isotopes, Ga-69 and Ga-71. The mass of Ga-69 is 68.9256 amu, and the mass of Ga-71 is 70.9247 amu. Use the atomic mass of gallium to determine the relative abundance of each isotope in a naturally occurring sample.

The figure is a representation of 50 atoms of a fictitious element with the symbol Nt and atomic number 120. Nt has three isotopes represented by the following colors: Nt-304 (red), Nt-305 (blue), and Nt-306 (green).

Neutron stars are believed to be composed of solid nuclear matter, primarily neutrons. (a) If the radius of a neutron is calculate its density in (b) Assuming that a neutron star has the same density as a neutron, calculate the mass in kilograms of a small piece of a neutron star the size of a spherical pebble with a radius of 0.10 mm.