Chemistry - chapter 9

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. [ Ga ]

[ Ar ]4s^23d^104p^1

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. [ As ]

[ Ar ]4s^23d^104p^3

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. [ Br ]

[ Ar ]4s^23d^104p^5

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. [ I ]

[ Kr ] 5s^24d^105p^5

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. [ Rb ]

[ Kr ]5s^1

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. [ Sn ]

[ Kr ]5s^24d^105p^2

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. [ Te ]

[ Kr ]5s^24d^105p^4

Within an electron configurations, what do symbols such as [Ne] and [Kr] represent?

[ Ne ] represents 1s^22s^22p^6 [ Kr ] represnets 1s^22s^22p^63s^23p^64s^23d^104p^6

Write electron configurations for each element. Use the symbol of the previous noble gas in brackets to represent the core electrons. [ Cs ]

[ Xe ]6s^1

How many 3d electrons are in an atom of each element? [ K ]

0

How many 3d electrons are in an atom of each element? [ As ]

10

How many 3d electrons are in an atom of each element? [ Zn ]

10

Write full electron configurations for each element [ Li ]

1s^22s^1

Write a full electron configuration and indicate the valence electrons and the core electrons for each element. [ B ]

1s^22s^22p^1

Write a full electron configuration and indicate the valence electrons and the core electrons for each element. [ N ]

1s^22s^22p^3

Write full electron configurations for each element [ N ]

1s^22s^22p^3

Write full electron configurations for each element [ Mg ]

1s^22s^22p^63s^2

Write full electron configurations for each element [ Ar ]

1s^22s^22p^63s^23p^6

Write full electron configurations for each element [ Ge ]

1s^22s^22p^63s^23p^64s^23d^104p^2

Write full electron configurations for each element [ Se ]

1s^22s^22p^63s^23p^64s^23d^104p^4

Write full electron configurations for each element [ Kr ]

1s^22s^22p^63s^23p^64s^23d^104p^6

Write full electron configurations for each element [ Sr ]

1s^22s^22p^63s^23p^64s^23d^104p^65s^2

Write a full electron configuration and indicate the valence electrons and the core electrons for each element. [ K ]

1s^22s^2sp^63s^23p^64s^1

Write a full electron configuration and indicate the valence electrons and the core electrons for each element. [ Sb ]

1s^2^2s^22p^63s^23p^64s^23d^104p^65s^24d^105p^3

How many 2p electrons are in an atom of each element? [ C ]

2

How many valence electrons are in each element? [ Ba ]

2

How many valence electrons are in each element? [ Be ]

2

How many 2p electrons are in an atom of each element? [ N ]

3

How many valence electrons are in each element? [ Al ]

3

How many 2p electrons are in an atom of each element? [ F ]

5

How many 2p electrons are in an atom of each element? [ P ]

6

How many 3d electrons are in an atom of each element? [ Fe ]

6

How many valence electrons are in each element? [ Se ]

6

Use the periodic table to identify the element with each electron configuration ( [Ar]4s^23d^104p^1 )

gallium

What is an emission spectrum? Use the Bohr model to explain why the emission spectrum of the hydrogen atom consists of distinct lines at specific wavelengths

An emission spectrum is the pattern of specific wavelengths of light that are emitted by specific elements when they are in an excited state. The Bohr model explains emission spectra at specific wavelengths as the result of an electron in a high-energy orbital relaxing down to a lower-energy state, with the excess energy given off as a photon of light with a quantized amount of energy

Explain the periodic trends in each chemical property ( atomic size )

Atomic size increases down a group because additional shells or layers of orbitals are added. Atomic size decreases across a period from left to right as the increase in positive charge on the nucleus exerts a stronger attraction on the electronic orbitals, pulling them closer to the nucleus and, therefore, shrinking the size of the atom.

Arrange the elements in order of increasing atomic size ( Fr, Sb, In, S, Ba, Se )

S<Se<Sb<In<Ba<Fr

Arrange the elements in order of increasing atomic size ( Cs, Sb, S, Pb, Se )

S<Se<Sb<Pb<Cs

Arrange the elements in order of increasing atomic size ( Ca, Rb, S, Si, Ge, F )

F<S<Si<Ge<Ca<Rb

Explain why Group 1 elements tend to form 1+ ions and Group 7 elements tend to form 1- ions

Group 1 elements form +1 ions because the electron configuration of the ion will match that of a noble gas. The group 7 elements form -1 ions for the same reason

Arrange the elements in order of increasing ionization energy ( Ga, In, F, Si, N )

In<Ga<Si<N<F

Explain the periodic trends in each chemical property ( metallic character )

Metallic character decreases as you move across a period from left to right and increases as you move down a group. This is consistent with the trends for ionization energy, since metals tend to lose electrons to form cations. The lower the ionization energy the more metallic the element.

Arrange the elements in order of increasing atomic size ( Sr, N, Si, P, Ga, Al )

N<P<Si<Al<Ga<Sr

Arrange the elements in order of increasing ionization energy ( Te, Pb, Cl, S, Sn )

Pb<Sn<Te<S<Cl

List the number of elements in periods 1 and 2 of the periodic table. Why does each period have a different number of electrons?

Period 1 consists of two elements within the 1s subshell. The S subshell has a maximum of two elements. Period 2 consists of eight elements within the 2s and the 2p subshells. The S subshell has a maximum of two elements, and the P subshell has a maximum of six elements for a combined total of eight elements

List the number of elements in periods 3 and 4 of the periodic table. Why does each period have a different number of electrons?

Period 3 consists of eight elements within the 3s and 3p subshells. The S subshell has a maximum of two elements, and the P subshell has a maximum of six elements for a combined total of eight elements. Period 4 consists of 18 elements within the 4s, 3d, and 4p subshells. The S subshell has a maximum of two elements, the d subshell has a maximum of ten elements, and the p subshell has a maximum of six elements for a combined total of 18 elements

Explain the difference between a Bohr orbit and a quantum-mechanical orbital

The Bohr model orbit is a circular orbit that maps the exact path an electron would make around a nucleus. The quantum-mechanical model, however has an orbital that is best described as a region that has the greatest probability for the location of an electron.

What is the difference between the ground state of an atom and an excited state of an atom?

The ground state is the lowest energy state of an atom in which all electrons are in the lowest possible energy orbital. The excited state of an atom is when an electron occupies an unstable higher energy orbital.

List some examples of the explanatory power of the quantum-mechanical model.

The quantum-mechanical model helps explain the chemical properties of the atoms, that is, their tendency to gain or lose electrons and how many electrons they gain or lose. It also explains periodic trends such as ionization energies and atomic radius

Explain the difference between valence electrons and core electrons

Valance electrons are the S and P electrons in the outermost shell. The core electrons are the inner electrons

Name the element in the third period ( row ) of the periodic table ( three valence electrons )

aluminum

Name the element in the third period ( row ) of the periodic table ( six 3p electrons )

argon

Name the element in the fourth period of the periodic table with ( five valence electrons )

arsenic or vanadium

Use the periodic table to identify the element with each electron configuration ( [Ne]3s^23p^5 )

chlorine

Explain the periodic trends in each chemical property ( ionization energy )

ionization energies increase going across a row in the periodic table from left to right because it is easier to remove electrons from metals to obtain a closed-shell electronic configuration. Nonmetals prefer to gain electrons to obtain the closed-shell configuration, so removing an electron would be expected to involve greater energy. Ionization energy decreases going down a column because the valence electrons are in higher- energy shells farther away from the nucleus and are easier to remove to form ions

Use the periodic table to identify the element with each electron configuration ( [Ar]4s^23d^6 )

iron

Name the element in the fourth period of the periodic table with ( a complete outer shell )

krypton

Name the element in the third period ( row ) of the periodic table ( two 3s electrons and no 3p electrons )

magnesium

List the outer electron configuration for each column in the periodic table [ 1A ]

ns^1

List the outer electron configuration for each column in the periodic table [ 2A ]

ns^2

List the outer electron configuration for each column in the periodic table [ 3A ]

ns^2np^1

List the outer electron configuration for each column in the periodic table [ 5A ]

ns^2np^3

List the outer electron configuration for each column in the periodic table [ 6A ]

ns^2np^4

List the outer electron configuration for each column in the periodic table [ 7A ]

ns^2np^5

List the outer electron configuration for each column in the periodic table [ 8A ]

ns^2np^6

List the outer electron configuration for each column in the periodic table [ 4A ]

ns^np^2

Use the periodic table to identify the element with each electron configuration ( [Kr]5s^1 )

rubidium

Name the element in the fourth period of the periodic table with ( a total of four 4p electrons )

selenium

Name the element in the third period ( row ) of the periodic table ( a total of four 3p electrons )

sulfur

Name the element in the fourth period of the periodic table with ( a total of three 3d electrons )

vanadium