Skip to main content
Indietro

General Chemistry: Periodic Atomic Properties and Electron Configuration

I pulsanti di controllo sono stati cambiati in modalità "navigazione".
1/20

Termini in questo insieme (20)

  • What is the significance of groups (columns) in the periodic table?
    Groups contain atoms with very similar chemical properties due to having the same number of valence electrons.
  • Who invented the periodic table and how are elements arranged?
    Dmitri Mendeleev invented the periodic table, arranging elements in order of increasing atomic number (Z).
  • What are periods in the periodic table?
    Horizontal rows in the periodic table, where elements show a repeating pattern of chemical properties.
  • Define core and valence electrons.
    Core electrons are in completed noble gas shells and do not affect chemical properties; valence electrons are in the outermost shell and determine chemical behavior.
  • Why are noble gas electron configurations considered stable?
    Because they have paired electrons and symmetrical, tight electron distributions, making them less reactive.
  • What drives the formation of ions in atoms?
    Atoms form ions by losing or gaining electrons to mimic the electron configuration of the nearest noble gas for stability.
  • What is the common charge formed by alkali metals (Group 1A)?
    Alkali metals typically form +1 charged cations by losing one valence electron.
  • How many valence electrons do alkaline earth metals (Group 2A) have and what charge do they form?
    They have two valence electrons and typically form +2 charged cations.
  • What is the typical charge and valence electron configuration of halogens (Group 7A)?
    Halogens have seven valence electrons and typically form -1 charged anions by gaining one electron.
  • How does atomic size change within a group and why?
    Atomic size increases down a group because electrons occupy higher energy shells farther from the nucleus.
  • How does atomic size change across a period and why?
    Atomic size decreases from left to right across a period due to increasing nuclear charge pulling electrons closer.
  • What is ionization energy and what does it indicate about an element?
    Ionization energy is the energy required to remove an electron; higher ionization energy means an element is less likely to form cations.
  • How does Coulomb's law relate to ionization energy?
    Closer opposite charges have stronger attraction, so valence electrons in smaller atoms are held more tightly, increasing ionization energy.
  • What is the relationship between ionization energy and the tendency to form cations?
    Elements with lower ionization energy more readily form cations; those with higher ionization energy are less likely to do so.
  • What is the abbreviated (condensed) electron configuration?
    A simplified electron configuration that uses the noble gas symbol in brackets to represent core electrons.
  • How do the number of valence electrons relate to group numbers in main group elements?
    For main group elements (except He), the number of valence electrons equals the group number.
  • What charge do Group 6A elements like Oxygen and Sulfur typically form?
    They typically form 2- charged anions by gaining two electrons.
  • What charge does Group 5A element Nitrogen typically form?
    Nitrogen typically forms a 3- charged anion by gaining three electrons.
  • What charge does Group 3A element Aluminum typically form?
    Aluminum typically forms a 3+ charged cation by losing three electrons.
  • What is the difference between core and valence electrons in terms of chemical properties?
    Core electrons do not affect chemical properties, while valence electrons determine an element's chemical behavior.