Atomic Structure and the Periodic Table Flashcards Preview

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Flashcards in Atomic Structure and the Periodic Table Deck (13):

What does an Atom consist of?

It consists of the nucleus and electrons. The nucleus is in the centre of the atom and the electrons are around the outside.


What charge does the nucleus have?

The nucleus has a positive charge due to the protons.


What does the nuclear symbol tell you?

It tells you its proton number and its mass number.


What is an element?

An element is a substance that is made up of atoms with the same number of protons in their nucleus.


What is an isotope?

An isotope are different forms of the same element and they have extra neutrons.


What is a compound?

A compound is a substance that is formed from two or more elements.


How are Chemical Changes shown?

They are shown using chemical equations.


What is a symbol equation and how do you balance a symbol equation?

Symbol Equations are used to show the symbols of formulas. The first stage of balancing an equation is that there must always be the same number of atoms on both sides. The second stage is that you balance the equation by putting numbers in front of the formulas that are needed.


What is the history of the atom?

Firstly, John Dalton described atoms as solid spheres. Then JJ Thompson concluded that atoms were not solid spheres. The new theory was known as the plum pudding model. In 1909 Ernest Rutherford and his students carried out the famous alpha particle scattering experiments. This led to the creation of the nuclear model of the atom.


What is the electronic structure?

The electronic structure rules are that Electrons always occupy shells. The lowest energy levels are always filled first. Only a certain amount of electrons are allowed in each shell.


How has the Periodic Table developed?

The Periodic Table has developed because in the early 1800s the elements were arranged by atomic mass. However in 1869 Dimitri Mendeleev developed the Periodic table as we know it today.


What are some properties of Group 1 metals?

One property is that they are reactive and they are soft metals. They all have one electron in their outer shell. They have low density.


What are the properties for group 7 metals?

They are non-metals and are less reactive than group 1 metals. They have higher melting and boiling points. They have higher relative atomic masses.