Chapter 5 Flashcards
Electronegativity and its trends
The value that shows how well an atom can hold on to shared electrons
Top to bottom- decreases
1) electrons further from the nucleus
2) increase in shielding effect
Left to right- increases
1) increase in nuclear charge
2) electrons are closer to the nucleus
Atomic Radii and their trends
The size of the atom
Left to right get smaller
Top to bottom gets bigger
Electron affinity and its trends
The energy change that accompanies the addition of an electron to an atom
Left to right- increases
1) electrons are closer to the nucleus
2) increase in nuclear charge
Top to bottom- decrease
1) electrons are further from the nucleus
2) increase in shielding effect
Ionic radii and its trends
The size of the ion
Positive ions are smaller than the neutral atom
Negative ions are larger than the neutral atom
Ionization energy and its trends
The energy needed to remove an electron
Left to right - increase
1) increase in nuclear charge
2) electrons are closer to the nucleus
Top to bottom- decrease
1) electrons are further from the nucleus
2) increase in shielding effect
Octet rule
Most stable in order
A full outermost energy level
Full outer sublevel
1/2 full sublevel
Periodic Law
Elements put in increasing atomic #
Periodic trends
1) atomic number = protons
2) electrons determine properties
elements within a group have the same number of valence electrons
Dobereiner (johann)
Developed triads
Groups of three elements that have similar chemical properties
Physic properties varied in a structured way aligned with their atomic masses
Then looked at melting and boiling points and saw as mass went up so did the melting and boiling points
Newlands (John)
Law of Octaves
Listed elements in order of increasing atomic mass
Found that elements fall in a pattern where the properties repeat at regular intervals
Every eight elements has similar properties to the first element
Assigned atomic number to elements
Mendeleev (Dmitri)
Father of periodic table
Based on about 60 elements
Identified periodic properties
Physical and chemical properties repeated when ordered by increasing atomic mass
Periodicity- tendency of properties to repeat at regular intervals
Arranged the periodic table based in increasing atomic mass
Modern periodic table
Based on increasing atomic number not atomic mass
Chalcogens
Oxygen-sulfur-selenium-tellurium-polonium
The factors of I.E and how they effect I.E
The larger the nuclear charge the greater the I.E
The greater the radius the lower the IE
The greater the shielding effect the lower the IE
An electron from a full or half full sublevel requires greater IE
