Chapter 7 Review Flashcards
Effective Nuclear Charge is equal to
Atomic number - Core electrons
Effective Nuclear Charge is smaller than the ________
Charge of the nucleus (Z)
In an isoelectric series, ionic charge _____ while nuclear charge _____
Decreases , increases
Chemical properties are determined by: . . .
The number of valence electrons and how strongly the valence electrons are attracted to the nucleus
Though electrons are attracted to the nucleus, the __________, also known as “shield” electrons “shield” the valence electrons from the force of the nucleus
core electrons
What is “S”?
“S” is the number of core electrons
What is “Z”?
“Z” is the atomic number of an atom
What is “Zeff”
“Zeff” is the effective nuclear charge of an atom
What is “Zeff” in terms of valence electrons?
“Zeff” is the charge “felt” by the valence electrons of an atom
Atomic radii is the . . .
Distance between the nucleus and outermost electron
The unit for Atomic radii is the . . .
Angstrom or “Å”
As the amount of valence electrons increases, the attraction of the nucleus decreases, causing the electrons to “spread out”. This means that Atomic radii . . . from left to right.
decreases
As we go step down rows, the Atomic radii . . . because the amount of electron shells is increasing
increases
The greater the Zeff, the . . .
greater the attraction of the nucleus
Because there are fewer electrons in a cation compared to the parent atom, a cation is . . . than the parent atom
smaller
Because there are more electrons in an anion compared to the parent atom, an anion is . . . than the parent atom
larger
The Zeff of cations is . . . than the Zeff of the parent atom
greater
The Zeff of anions is . . . than the Zeff of the parent atom
less
In an isometric series, Atomic radii . . . with an increasing nuclear charge
decreases
In an isoelectric series, the largest ion will have the . . . number of protons
smallest
In an isoelectric series, the smallest ion will have the . . . number of protons
largest
An isoelectric series is a series of . . .
ions with the same number of electrons
Ionization energy is . . .
the minimum energy required to REMOVE one electron from an atom or ion
Ionization energy makes . . .
cations
Second ionization energy is always . . . than first ionization energy
greater
The correct way to show the first ionization energy of an atom (X) is . . .
X –> X(+) + e(-)
There is a sharp increase in ionization energy when you . . .
remove a core electron
For transition metals, if s and p orbitals have electrons, ___ electrons are removed first, then ___ electrons, before ___ electrons
p, s, and d
The exception groups for ionization energy are groups ___ and ___
3A and 6A
The more the amount of valence electrons, the easier it is to remove one, which means that ionization energy . . . from left to right
increases
As we move from top to bottom of the table of elements, valence electrons are farther and farther away, making it easy to remove one. This means that ionization energy . . . from top to bottom.
decreases
Electron Affinity’s symbol is ___
ΔE
Electron Affinity is . . .
The CHANGE in energy to ADD one electron to form an ANION
The more negative the Electron Affinity, the . . .
more stable the anion
The more stable the anion, . . .
the greater attraction between an atom and the added electron
If the Electron Affinity is positive, . . .
the less stable the anion
The correct way to show the Electron Affinity of an atom (X) is . . .
X + e(-) –> X(-)
The most non-metallic
elements have the . . . values
most negative
Groups where the electron affinities are near positive are Groups ___, ___, and ___
2A, 5A, and 8A
From left to right, electron affinity . . .
increases
From top to bottom, electron affinity . . .
stays the same
The period with generally the largest electron affinity is . . .
period 3
Electron Negativity’s symbol is . . .
EN
Electron Negativity is . . .
the ability of an atom, that is bonded to
another atom, to attract electrons to itself
Electron Negativity . . . from left to right
increases
Electron Negativity . . . from top to bottom
decreases
The exception to the Electron Negativity is . . .
Group 8A
Metals have . . . ionization energies
low
Metal oxides are . . .
bases, which
1. react with acids to form salt
and water
2. dissolve in water and react to form metal hydroxides.
Metal oxide + acid –>
salt + water
Metal oxide + water –>
metal hydroxide
Alkali metals have low . . .
densities, melting points, and ionization energies
Compared to Alkali metals, Alkaline metals have higher . . .
densities, melting points, and ionization energies
As you go down the group of Alkaline metals, ________ tends to increase
reactivity
The melting points of nonmetals are generally . . . than those of metals
lower
These elements occur naturally as diatomic
H, N, O, F, Cl, Br, and I
Nonmetals tend to . . .
gain electron and become anions
Nonmetal oxides are . . .
acids, which
1. dissolve in basic solutions to form a salt
and water
2. dissolve in water react to form acids
nonmetal oxide + base –>
salt + water
nonmetal oxide + water –>
oxyacid
Hydrogen is a . . .
nonmetal gas
Hydrogen typically likes to form . . .
the +1 ion
The ionization energy of Hydrogen is . . . than the Alkali metals
higher
When Hydrogen is part of an ionic compound with a metal, Hydrogen becomes a . . .
H(-)
Ionic compounds with H(-) are called . . .
Metal hydrides
Under extreme pressure, Hydrogen can . . .
act like a metal, conduct electricity, and conduct heat
One or more forms of a chemical element that occur in the same
physical state are known as . . .
Allotropes
Allotropes form because of the . . .
different ways atoms may be bonded together
Allotropes may display . . . chemical and physical properties
very different
In response to changes in pressure,
temperature, and exposure to light, elements may change ________
Allotrpoes
What elements are all nonmetals and have highly negative electron affinities?
F, Cl, Br, and I
What element removes electrons from almost any substance it contacts (very
exothermic), including water, and is very reactive?
Fluorine
The halogens react directly with most metals to form . . .
Ionic halides
The halogens also react with diatomic H to form gaseous
Hydrogen halide compounds
The Noble Gases are . . .
gaseous, monatomic nonmetals
Noble gases are very unreactive because they have full . . .
s and p subshells
The only noble gases to form chemical compounds are . . .
the heaviest because of the lower ionization energies
Metals tend to ____ electrons
lose
Metals tend to lose electrons because of . . .
low ionization energies
Nonmetals tend to ____ electrons
gain
Nonmetals tend to lose electrons because of . . .
high electron affinities
Compounds formed between metals and nonmetals tend to be _____
ionic
An element’s reactivity is characterized by its . . .
metallic character
Metals are on the left side of the Table while Nonmetals are on the right side of the Table, which means Metallic Character _________ from left to right
decreases
Because Ionization
energy decreases down a
group, making it easier for an atom to lose an electron, Metallic Character _________ from top to bottom
increases
Group 1A is
Alkali Metals
Group 2A is
Alkaline Earth Metals
Group 8A is
Noble Gases
Group 7A is
The Halogens
Group 6A is
The Chalcogens
Group 1A elements include . . .
Li, Na, K, Rb, Cs, and Fr
Group 2A elements include . . .
Be, Mg, Ca, Sr, Ba, and Ra
Group 8A elements include . . .
He, Ne, Ar, Kr, Xe, and Rn
Group 7A elements include . . .
F, Cl, Br, I, and At
Group 6A elements include . . .
O, S, Se, Te, and Po
