Chemistry Chapter 5 Flashcards
what year did the international congress of chemistry agree on method of determining and standardizing atomic mass
1860
who organized elements in order of increasing atomic mass; found elements had similar properties at regular intervals
left empty spaces for elements not yet discovered at his time
Medelev
what are elements grouped together in ?
families
who and what year did a scientist determine atomic numbers for elements and arranged the periodic table according to atomic number
1911 and Mosely
the physical and chemical properties of the elements are functions of their atomic numbers
periodic law
arrangement of elements in order of their atomic numbers so that elements with similar properties fall in the same group
the modern periodic table
discovery and synthesis of new elements
modern additions to the periodic table
unreactive elements in our atmosphere
noble gases
group 1 and 2 elements are in what block?
s- block
alkali metals
s block
alkali earth metals
s block
Li, Na, K, Rb, Cs, Fr
group 1 alkali metals
all soft, silvery metals
group 1 alkali metals
melting point> boiling point of water
group 1 alkali metals
one electron in outer shell
group 1 alkali metals
very reactive (not found free in nature)
group 1 alkali metals
Be, Mg, Ca, Sr, Ba, Ra
group 2 alkali earth metals
all silvery metals but harder and stronger than another group
group 2 alkali earth metals
two electrons in outer shell
group 2 alkali earth metals
re-activity
group 2 alkali earth metals
what block is group 3-12
d-block elements
what are group 3-12 called
transition elements and d-block elements
all metals
groups 3-12 transition metals
have properties of metals
- less reactive
- high luster
- good conductivity
groups 3-12 transition metals
what block is group 13-18
p-block elements
properties vary
group 13-18 p-block
some non-metals
some metalloids
some metals
group 13-18 p-block
what block are halogens in?
p-block
what group is halogens in?
group 17
F, Cl, Br, At
group 17 halogens
all non-metals
group 17 halogens
very reactive
group 17 halogens
7 electrons in outer shell
group 17 halogens
what block is noble gases in?
p-block
what group are the noble gases in
group 18
He, Ar, Kr, Xe, Rn
group 18 noble gases
all non-metals and gases
group 18 noble gases
8 electrons in outer shell/except helium
group 18 noble gases
non-reactive
group 18 noble gases
what block is the lanthanide series in?
f-block
What block is the actinide series in?
f-block
contains radioactive elements
f-block actinide series
natural and man-made
f-block actinide series
atomic radii as a periodic property
- _______ across periods due to ___________ positive charge of the nuclei
- _______ down a group due to ___________ number of levels
decreases, increasing
increase, increasing
minimum amount of energy to remove an electron
A+energy–>Apositive+electron
ionization energy
loosing electron makes ion more _____
positive
ionization energy as a periodic property:
- ______ across the periods due to _____ nuclear change
- ______ down the column due to distance from the nucleus
increases, increasing
decreases
removing electron from positive ions
- each _____ electron removed from an ion feels an _______ stronger effective nuclear charge-> ionization energy _____
- a _____ ionization energy ______ occurs when a electron is removed from an inner, stable level
successive, increasing, increases
large, increase
energy released when an atom acquires an electron
A+electron–>Anegative+energy
electron affinity
electron affinity
when energy is released=__________ value
negative
- values become ____ negative across the periods
- values become ____ negative down a column
more
less
positive ion
cation
negative ion
anion
cation: _____ radius compared to atom due to loss of outer shell electron and _____ nuclear pull
smaller, increased
anion: _____ radius compared to atom due to ______ nuclear pull and ______ electron cloud
large, decreased, increasing
of electrons in outer shell
valence electrons
valence electrons group 1 =? group 2=? group 13=? group 14=? group 15=? group 16=? group 17=? group 18=?
1 2 3 4 5 6 7 8 (except He)
measure of the ability of an atom in a compound to attract electrons
scale=0-4
0=____ ability to attract
4=____ ability to attract
electronegativity
lowest
greatest
electronegativity
____ across the period
____ down the column
increases
decrease
Mendeleev organized the chemical elements based on their
properties
A horizontal row in the period table is called a
period
the physical and chemical properties of the elements are functions of their atomic number
periodic law
An element with the general electron configuration ns^2np^1 for its outermost electrons would be in group
13
When a carbon atom is in its ground state, how many electrons does it have in its outermost shell?
4
Which of the following elements is most similar in behavior to calcium?
a. magnesium
b. sodium
c. sulfur
d. chlorine
magnesium
Which periodic group or family of elements is not correctly matched with its common family name?
a. Group 2: alkaline-earth metals
b. Group 3: alkali metals
c. Group 17: halogens
d. Group 18: noble gases
alkali metals
the electron configurations of main group elements end in
s and p orbitals
Which of the following elements is a transition metal?
a. calcium
b. iron
c. sodium
d. sulfur
iron
all the alkali metal elements are found on the periodic table in
group 1
a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called
electronegativity
which of the following elements has the greatest atomic radius?
a. Al
b. S
c. Si
d. C
Al
largersmaller
which of the following elements has the lowest electronegativity
a. C
b. F
c. Li
d. O
Li
lower–electronegativity–>higher
which of the following elements has the greatest ionization energy?
a. Ga
b. K
c. Bi
d. As
As
low—>ionization—>higher
which of the following elemnts has an electron affinity of 0kJ/m
a. Br
b. As
c. Ar
d. I
Ar
elements have full outer energy levels when they are in the ground state
noble gases
in which period is an element that has the electron configuration 1s^2 2s^2 2s^6 3s^2 3p^6 3d^10 4s^2 4p^1
period 4
which of the following elements is not a metal?
a. H
b. K
c. Na
d. Fr
H
for atoms of p-block elements, the total number of electrons in the highest occupied level is equal to the…
group number minus 10
as electrons add to s and p sublevels in the same main energy level they are pulled closer to the more highly charged nucleus, causing
atomic radii to decrease in size
which electron configuration would result in the largest negative electron affinity?
a. He 2s^1
b. He 2s^2 2p^2
c. He 2s^2 2p^3
d. He 2s^2 2p^5
He2s^2 2p^5
In forming an ion, from which sublevel would an atom of nickel lose electrons first?
4s
which one of the following groups contains atoms that, in compounds, have the lowest attraction for electrons
a. group 1
b. group 2
c. group 16
d. group 17
group 1
which ionization energy is generally the largest
fourth ionization energy
the metalloids are located on the period table between
nonmetals and metals
Name the element in group 1 with the most negative (less positive) electron affinity
Li
Name the element in Group 17 with the lowest ionization energy
At
Name the element in period 2 with the largest atomic radius
Li
Name the element in group 15 with the smallest electronegativity
Bi
Name the element in period 3 most likely to form an ion with a 2+ charge
Mg
electron affinity values tend to become more or less negative?
more
ionization energy values tend to become larger or smaller
larger
atomic radii tend to become larger or smaller
smaller
how will the radius of a magnesium atom compare to the radius of the magnesium ion (Mg+2), explain your answer
Mg>Mg+2
what does ionization energy measure
amount of energy required to remove an electron
why is F considered to be the most reactive nonmental?
7electrons in outer shell-desperate to get 1 smallest radii- less shells to exert pull on electron highest electronegativity
how can you use the periodic table to predict valence eletrons
group 1= 1
group 2= 2
group 13=3
