C2 Flashcards
(40 cards)
What are the significant models for ordering elements in the periodic table?
Development of the elements
Various models have been proposed throughout history to organize elements based on their properties.
How are the elements ordered in the periodic table?
By increasing atomic number
The periodic table arranges elements in order of their atomic numbers, which corresponds to the number of protons in an atom.
Define a group in the periodic table.
A column of elements with similar properties
Elements in the same group typically exhibit similar chemical behaviors.
Define a period in the periodic table.
A row of elements with increasing atomic numbers
Each period represents a new principal energy level for the electrons.
How is electronic structure linked to the periodic table?
It determines the position of elements
The electronic structure influences an element’s chemical properties and its placement in the periodic table.
What characterizes noble gases?
They are unreactive
Noble gases have full outer electron shells, making them stable and non-reactive.
Name the first three elements in Group 1.
Lithium, Sodium, Potassium
These elements are known as alkali metals.
Describe the Group 1 metals.
They have low densities
This characteristic allows some of them to float on water.
Write a word equation for the reaction of Group 1 metals with water.
Metal + Water → Metal Hydroxide + Hydrogen
This reaction illustrates the formation of hydrogen gas and a metal hydroxide.
How are elements arranged in groups and periods in the periodic table?
By similar properties in groups and increasing atomic number in periods
This arrangement allows for the prediction of element behavior.
Why was the periodic table a breakthrough in ordering elements?
It provided a systematic way to categorize elements
The periodic table revealed relationships among elements based on their properties.
How do the electronic structures of metals and non-metals differ?
Metals have fewer electrons in their outer shell compared to non-metals
This difference affects their reactivity and bonding behavior.
Why are noble gases unreactive?
They have full outer electron shells
This stability results in a lack of tendency to form chemical bonds.
What is the trend in boiling points of noble gases?
They increase with atomic number
As the atomic size increases, the boiling point rises due to increased van der Waals forces.
Why do elements in Group 1 react similarly?
They have the same number of electrons in their outer shell
This similarity leads to analogous chemical properties.
What happens to Group 1 metals when they react with water?
They produce hydrogen gas and metal hydroxides
This reaction is exothermic and can be vigorous.
How has the ordering of elements changed over time?
New discoveries led to reclassification
Advances in atomic theory and technology have refined the periodic table.
How does the electronic structure of metals and non-metals affect their reactivity?
Metals tend to lose electrons, while non-metals tend to gain electrons
This electron transfer is fundamental to chemical reactions.
How can the periodic table be used to predict electronic structure and reactions?
By analyzing trends and positions of elements
The table provides insights into valence electrons and expected chemical behavior.
Predict the electronic structure of stable ions for the first 20 elements.
Stable ions have full outer shells
This typically results in ions with configurations similar to noble gases.
Illustrate the reactions of Group 1 metals with balanced symbol equations.
2Na + 2H2O → 2NaOH + H2
This equation shows sodium’s reaction with water.
How do Group 1 metals form ions?
They lose one electron to form +1 charged ions
This loss of an electron results in a stable electronic configuration.
What safety precautions are necessary when handling Group 1 metals?
Store under oil to prevent reactions with moisture
Group 1 metals are highly reactive, particularly with water and air.
can explain in terms of electronic
structure how the elements are arranged
in the periodic table.
Nuclear Charge Increases: The nucleus becomes more positively charged because each proton carries a positive charge.
Electrons Increase: To maintain neutrality, more electrons are added to the atom.
